化学实验报告-英文版-2
化学实验报告 英文版
化学实验报告英文版Chemical Experiment ReportAbstract:This report presents the findings and analysis of a chemical experiment conducted to investigate the effects of temperature on the rate of reaction between hydrochloric acid (HCl) and sodium thiosulfate (Na2S2O3). The experiment involved varying the temperature of the reactants and measuring the time taken for the reaction to occur. The results indicate a clear correlation between temperature and reaction rate, with higher temperatures leading to faster reactions.Introduction:Chemical reactions are influenced by various factors, including temperature, concentration, and catalysts. The purpose of this experiment was to examine the impact of temperature on the rate of a chemical reaction. The reaction between hydrochloric acid and sodium thiosulfate was chosen due to its well-documented reaction kinetics.Methodology:The experiment was conducted using a simple setup consisting of a conical flask, a stopwatch, and a thermometer. Initially, 50 mL of 1 M hydrochloric acid was poured into the flask, followed by the addition of 10 mL of 0.1 M sodium thiosulfate. The stopwatch was started as soon as the sodium thiosulfate was added, and the time was recorded when the solution turned opaque due to theformation of a yellow precipitate. The experiment was repeated at different temperatures by immersing the flask in water baths maintained at specific temperatures.Results and Discussion:The experiment was carried out at four different temperatures: 20°C, 30°C, 40°C, and 50°C. The average reaction times at each temperature were recorded and are presented in Table 1 below:Temperature (°C) Reaction Time (s)20 12030 9040 7050 50Table 1: Average reaction times at different temperaturesFrom the results, it is evident that as the temperature increased, the reaction time decreased. This indicates that higher temperatures accelerate the rate of the reaction between hydrochloric acid and sodium thiosulfate. The relationship between temperature and reaction rate can be explained by the collision theory. According to this theory, particles must collide with sufficient energy to overcome the activation energy barrier for a reaction to occur. As temperature increases, the average kinetic energy of the particles also increases, leading to more frequent and energetic collisions.Furthermore, the reaction between hydrochloric acid and sodium thiosulfate isexothermic, meaning it releases heat. As the reaction progresses, the released heat raises the temperature of the solution, further increasing the reaction rate. This positive feedback mechanism contributes to the observed trend of faster reactions at higher temperatures.Conclusion:In conclusion, this experiment demonstrates the significant influence of temperature on the rate of the reaction between hydrochloric acid and sodium thiosulfate. As temperature increases, the reaction time decreases due to more energetic collisions and the exothermic nature of the reaction. These findings have practical implications in various fields, such as industrial chemistry and environmental science, where controlling reaction rates is crucial.Further research could explore the effect of temperature on other chemical reactions and investigate the specific activation energy values for different reactants. Additionally, studying the impact of other factors, such as concentration and catalysts, on reaction rates would provide a comprehensive understanding of chemical kinetics.。
化学实验报告英语
化学实验报告英语Chemical Experiment ReportIntroductionChemical experiments play a crucial role in the field of science and technology. They provide valuable insights into the properties and behavior of various substances. In this report, we will discuss a series of chemical experiments that were conducted in a laboratory setting. The experiments aimed to explore the effects of different variables on the reaction rate and product formation. Experiment 1: Reaction Rate and ConcentrationIn this experiment, we investigated the relationship between reaction rate and concentration. We prepared a solution of hydrochloric acid and sodium thiosulfate. By varying the concentration of sodium thiosulfate and keeping the concentration of hydrochloric acid constant, we observed the time taken for the solution to turn cloudy. As expected, we found that a higher concentration of sodium thiosulfate resulted in a faster reaction rate. This experiment demonstrated the importance of concentration in determining the rate of a chemical reaction.Experiment 2: Temperature and Reaction RateTemperature is another crucial factor that influences reaction rates. To study this, we heated a solution of potassium permanganate and oxalic acid to different temperatures. We then measured the time taken for the solution to change color. The results showed that an increase in temperature led to a significantincrease in the reaction rate. This can be attributed to the fact that higher temperatures provide more energy to the reacting particles, increasing their collision frequency and the likelihood of successful collisions.Experiment 3: Catalysts and Reaction RateCatalysts are substances that can speed up a chemical reaction without being consumed in the process. In this experiment, we examined the effect of a catalyst on the decomposition of hydrogen peroxide. We added a small amount of manganese dioxide to a solution of hydrogen peroxide and observed the release of oxygen gas. The presence of the catalyst facilitated the decomposition of hydrogen peroxide, leading to a faster reaction rate. This experiment highlighted the role of catalysts in enhancing reaction rates and their importance in various industrial processes.Experiment 4: pH and Product FormationThe pH of a solution can significantly influence the formation of products in a chemical reaction. To investigate this, we conducted an experiment involving the reaction between acetic acid and sodium bicarbonate. We varied the pH of the acetic acid solution by adding different amounts of sodium hydroxide. We then measured the volume of carbon dioxide gas produced. The results indicated that a higher pH resulted in a greater volume of carbon dioxide gas. This experiment emphasized the impact of pH on the formation of products in chemical reactions.ConclusionChemical experiments provide valuable insights into the behavior and properties of substances. Through the experiments discussed in this report, we explored the effects of concentration, temperature, catalysts, and pH on reaction rates and product formation. These experiments demonstrate the importance of understanding the factors that influence chemical reactions and their applications in various fields, including pharmaceuticals, materials science, and environmental studies. By furthering our knowledge in this area, we can continue to make advancements in the field of chemistry and contribute to the development of new technologies.。
化学实验报告 英文
化学实验报告英文Chemistry Experiment ReportIntroduction:In the field of science, experiments play a crucial role in deepening our understanding of various phenomena. This report aims to present the findings and observations from a recent chemistry experiment conducted in the laboratory. The experiment focused on the reaction between two chemicals and explored the effects of different variables on the reaction rate.Experimental Procedure:The experiment began by carefully measuring and preparing the required chemicals: sodium hydroxide (NaOH) and hydrochloric acid (HCl). These chemicals were chosen due to their well-known reaction, which produces salt and water. The experiment aimed to investigate how factors such as concentration, temperature, and catalysts influenced the reaction rate.To start the experiment, a fixed volume of NaOH solution was poured into a conical flask. The concentration of NaOH was varied in different trials, ranging from 0.1 M to 1.0 M. The flask was placed on a magnetic stirrer to ensure uniform mixing. Then, a burette was used to add a fixed volume of HCl solution to the flask. The reaction was monitored by observing the formation of a white precipitate, indicating the completion of the reaction.Results and Discussion:The experiment revealed several interesting findings. Firstly, it was observed thatas the concentration of NaOH increased, the reaction rate also increased. This can be attributed to the higher number of NaOH particles available to react with HCl, leading to more frequent collisions and faster reaction kinetics. Furthermore, the effect of temperature on the reaction rate was investigated. It was found that as the temperature increased, the reaction rate also increased. This can be explained by the kinetic theory of gases, which states that at higher temperatures, particles possess greater kinetic energy and move more rapidly. Consequently, more collisions occur, resulting in a faster reaction rate.The influence of catalysts on the reaction rate was also examined. A small amount of catalyst, in the form of manganese(IV) oxide (MnO2), was added to the reaction mixture. It was observed that the presence of the catalyst significantly increased the reaction rate. Catalysts provide an alternative reaction pathway with lower activation energy, allowing the reaction to proceed more rapidly.Conclusion:In conclusion, this experiment provided valuable insights into the factors affecting the reaction rate between NaOH and HCl. The concentration of the reactants, temperature, and the presence of catalysts were identified as key variables influencing the rate of the reaction. Understanding these factors is crucial in various industrial processes where reaction rates play a vital role.It is important to note that this experiment focused on a specific reaction and variables. Further research could explore the effects of other factors, such aspressure and surface area, on the reaction rate. Additionally, investigating the reaction kinetics using mathematical models could provide a more comprehensive understanding of the underlying mechanisms.Overall, this experiment highlights the significance of chemistry in unraveling the mysteries of the natural world. By conducting experiments and analyzing the results, scientists can uncover fundamental principles that govern chemical reactions, paving the way for advancements in various fields, including medicine, energy, and materials science.。
化学实验报告常见英文
Experiment Title: Synthesis of Ethanol from EthanolamineDate: [Date]Objective:The objective of this experiment was to synthesize ethanol from ethanolamine using the dehydration reaction. Ethanolamine is a compound with the molecular formula NH2CH2CH2OH, and it can be dehydrated to produce ethanol (CH3CH2OH) and ammonia (NH3).Materials:- Ethanolamine (NH2CH2CH2OH)- Sulfuric acid (H2SO4)- Concentrated sulfuric acid- Ethanol- Sodium chloride (NaCl)- Distilled water- Sodium hydroxide (NaOH)- Sodium sulfate (Na2SO4)- Potassium permanganate (KMnO4)- Barium chloride (BaCl2)- Distillation apparatus- Reaction vessel- Round-bottom flask- Condenser- Thermometer- Test tubes- Pipettes- Weighing scale- Stirring rod- Safety goggles- Gloves- Lab coatProcedure:1. Measure 5 g of ethanolamine using a weighing scale and transfer it toa round-bottom flask.2. Add 5 mL of concentrated sulfuric acid to the flask and stir the mixture thoroughly.3. Place the flask in a water bath and heat it to 60°C for 2 hours. This will facilitate the dehydration reaction.4. After 2 hours, remove the flask from the water bath and allow it to cool to room temperature.5. Transfer the reaction mixture to a distillation apparatus. The distillation apparatus consists of a round-bottom flask, a condenser, and a receiving flask.6. Heat the mixture to approximately 78°C, which is the boiling point of ethanol. Ethanol will vaporize and be collected in the receiving flask.7. Collect the distillate and transfer it to a test tube. Add 5 mL of water to the test tube and observe the appearance of the liquid.8. To identify the presence of ammonia, add a few drops of potassium permanganate to the test tube. If the solution turns brown, it indicates the presence of ammonia.9. To confirm the purity of the ethanol, add a few drops of barium chloride to the test tube. If a white precipitate forms, it indicates the presence of sodium chloride, which was used as a catalyst in the reaction.10. Dispose of the waste products and clean the equipment.Results:- The reaction mixture was heated to 60°C for 2 hours, and the distillation was performed at approximately 78°C.- Ethanol was collected in the receiving flask, and the distillate was observed to be a clear liquid.- A brown color was observed in the test tube when potassium permanganate was added, indicating the presence of ammonia.- A white precipitate formed when barium chloride was added, indicating the presence of sodium chloride.Discussion:The dehydration reaction of ethanolamine to produce ethanol was successfully achieved in this experiment. The reaction mixture was heated to 60°C for 2 hours to facilitate the dehydration process. Ethanol was collected in the receiving flask, and the distillate was observed to be a clear liquid, indicating the successful synthesis of ethanol.The presence of ammonia was confirmed by the brown color observed when potassium permanganate was added. This suggests that the dehydration reaction also produced ammonia as a byproduct.The formation of a white precipitate when barium chloride was added confirms the presence of sodium chloride, which was used as a catalyst in the reaction. The sodium chloride did not affect the purity of the ethanol product.Conclusion:The objective of synthesizing ethanol from ethanolamine using the dehydration reaction was successfully achieved in this experiment. Ethanol was produced, and the purity of the product was confirmed by observing the color changes and precipitate formation. This experiment provided a practical approach to understanding the dehydration reaction and its application in the synthesis of organic compounds.。
实习报告英文版
实习报告英文版标题：Internship ReportInternship ReportThe purpose of this report is to provide a comprehensive overview of my internship experience at [Insert Company Name], specifically from [Insert Start Date] to [Insert End Date]. The internship has given me a valuable opportunity to gain practical experience in the field of [Insert Field of Study], and has allowed me to develop professional skills and gain an understanding of the day-to-day operations of a successful organization.During my internship, I was assigned to the [Insert Department] department under the supervision of [Insert Supervisor's Name]. My primary responsibilities included [Insert Responsibilities], which were conducted in a challenging yet rewarding environment.My work involved tasks such as [Insert Specific Tasks], whichhelped me to gain a better understanding of the various aspects of the job. I found that the most difficult part of the internship was [Insert Difficulty], but through perseverance and hard work, I was able to overcome this challenge.The highlight of my internship was [Insert Highlight], which taught me [Insert Lesson/Insight]. I also learned that [Insert Other Lesson/Insight], which will help me in my future career. Overall, I am very pleased with my internship experience. The opportunity to apply my academic knowledge in a real-world setting has been invaluable. I have learned skills such as [Insert Skills Learned], which will enhance my future employability.I would like to express my gratitude to [Insert Company Name] and especially to [Insert Supervisor's Name] for their guidance and support throughout my internship. I would also like to thank the other members of the team for their assistance and hospitality.In conclusion, this internship has been an excellent learningexperience, and I am grateful for the opportunity to have worked in such a professional and stimulating environment. I am confident that the skills and knowledge I have gned during this time will enhance my future career prospects.ELISA 英文版实验报告一、实验目的本实验旨在学习和掌握ELISA（酶联免疫吸附试验）方法，了解其在临床诊断、生物研究等方面的应用。
化学性质实验报告
糖、氨基酸和蛋白质的鉴定糖类化合物：又称碳水化合物，是多羟基醛或多羟基酮及其缩聚物和某些衍生物的总称，一般由碳、氢与氧三种元素所组成。
实验目的：（1）进一步了解糖的化学性质；（2）掌握鉴定糖的方法及其原理。
（一）-萘酚试验（molish)糖类化合物一个比较普遍的定性反应是molish 反应。
即在浓硫酸存在下，糖与-萘酚(molish试剂）作用生成紫色环。
实验方法取3支试管，编号，分别加入 ml %的各待测糖水溶液，滴入2滴molish 试剂（ -萘酚的乙醇溶液），摇匀。
把试管倾斜450，沿管壁慢慢加入约1ml 浓硫酸（切勿摇动），小心竖直后仔细观察两层液面交界处的颜色变化。
硫酸在下层,试液在上层样品：葡萄糖、蔗糖及淀粉解释:糖被浓硫酸脱水生成糠醛或糠醛衍生物，后者进一步与-萘酚缩合生成紫红色物质，在糖液和浓硫酸的液面间形成紫色环。
（二） fehling试验（1）实验原理fehling试剂：含有硫酸铜和酒石酸钾钠的氢氧化钠溶液。
硫酸铜与碱溶液混合加热，生成黑色的氧化铜沉淀。
若同时有还原糖存在，则产生黄色或砖红色的氧化亚铜沉淀。
为防止铜离子和碱反应生成氢氧化铜或碱性碳酸铜沉淀，fehling试剂中需加入酒石酸钾钠，它与cu2＋形成的酒石酸钾钠络合铜离子是可溶性的络离子。
（2）操作方法取4支试管，编号，分别加入fehling试剂i和ii 各。
摇匀并置于水浴中微热后，分别加入5滴待测糖溶液，振荡后置于沸水浴中加热2 ~ 3min，取出冷却，观察颜色变化及有无沉淀析出。
fehling试剂 i：称取 g硫酸铜溶于100 ml蒸馏水中, 得淡蓝色的 fehling试剂 i。
fehling试剂 ii：将17g酒石酸钾钠溶于20ml热水中，然后加入20 ml 含5 g naoh的水溶液，稀释至100 ml得无色透明的fehling试剂 ii。
样品：葡萄糖、果糖、蔗糖及麦芽糖解释: 硫酸铜与碱溶液混合加热，生成黑色的氧化铜沉淀。
实验报告英文版
The determination of nitrogen content in the ammonium salt(Formaldehyde method)一、The experiment purpose1、To study the application of acid-base titration2、Master the formaldehyde method principle and the method for determination of nitrogen content in the ammonium salt3、The use of master the volumetric flask and pipet二、The experimental principleBecause NH4 acid is too weak to directly with NaOH standard solution titration, we usually using formaldehyde is transformed into titratable acid:4NH4++6HCOH=(CH2)6N4H++3H++6H2OProducts, hydrogen ions and (CH2)6N4H+ can be directly for accurate titration,titration product (CH2)6N4 is weak alkaline, so using phenolphthalein as indicator.According to the volume of the consumption of sodium hydroxide, may be calculated in proportion of nitrogen content in the ammonium salt:w(N)=C(NaOH)·V(NaOH)·M/m×100%三、Instruments and reagentsEquipment and materials:The alkali type buret(50ml)，Conical flask(250ml)，Volumetric flask(100ml)，pipette(20ml)，Measuring cylinder(10ml)，A beaker(100ml)，Analytical balance，Glass rodDrugs and reagents:Sodium hydroxide standard solution(0.1083mol/L),formaldehyde(40%)，phenolphthalein(2g/L ethanol solution),Samples of ammonium sulfate(S).四、The experimental steps1、Accurately according to 0.60 ~ 0.85 g samples of ammonium sulfate in 50 ml beaker, add right amount water dissolves directly transferred to the 100 ml volumetric flask and constant volume, shake a backup.2、Assimilation in sodium hydroxide standard solution to Alkali type buret after wash and embellish it.3、Accurately move 20 ml of the solution into the clean conical flask, add 10 ml of neutral formaldehyde solution and 1 drop of phenolphthalein indicator,shake the solution and let stand for 1 minutes, to the solution with sodium hydroxide standard solution titration is not fade reddish and maintain half minutes,as it to the end.4、Observe and record the volume of consumption of sodium hydroxide5、Parallel determination of three times, calculate the nitrogen content in the sample and the relative average deviation dr(≤0.3%)W(N)=(20.99%+21.01%+21.01%)/3=21.00%d=(0.01%+0.01%+0.01%)/3=0.01%dr=d/w(N)=0.01%/21.00%×100%=0.05%.。
化学实验报告英文版
Title: Synthesis of Ethyl Acetate from Ethanol and Acetic AcidDate: [Date of Experiment]Student Name: [Your Name]Lab Section: [Your Lab Section Number]Objective: The objective of this experiment was to synthesize ethyl acetate, a volatile organic compound, by the esterification of ethanol and acetic acid. This reaction is a classic example of a nucleophilic acyl substitution reaction, where the alcohol attacks the carbonyl carbon of the acid to form the ester.Introduction:Esters are organic compounds derived from carboxylic acids by the replacement of the hydroxyl group with an alkyl or aryl group. Ethyl acetate is a widely used solvent in the pharmaceutical, food, and perfume industries due to its pleasant smell and volatility. The synthesis of ethyl acetate is typically achieved through the esterification reaction between acetic acid and ethanol in the presence of an acid catalyst.Materials:- Ethanol (CH3CH2OH)- Acetic acid (CH3COOH)- Concentrated sulfuric acid (H2SO4) - Catalyst- Sodium chloride (NaCl) - Dehydrating agent- Water - Solvent- Distillation apparatus- thermometer- glassware (beakers, flasks, etc.)- pH meterProcedure:1. Preparation of Reactants:- Measure 10 mL of ethanol and 10 mL of acetic acid into a round-bottom flask.- Add 1 mL of concentrated sulfuric acid as a catalyst.- Swirl the flask gently to mix the contents.2. Heating and Stirring:- Place the flask on a hot plate and heat the mixture to approximately 50-60°C. Maintain the temperature for about 30 minutes, ensuring the mixture is well-stirred.- The reaction is exothermic, so be cautious when heating.3. Adding Sodium Chloride:- After the reaction time, remove the flask from the heat.- Add a small amount of sodium chloride to the mixture. This helps to remove water from the reaction mixture, which can be a byproduct of the reaction.4. Observation:- The reaction mixture should now have a noticeable odor of ethyl acetate.- The mixture may also turn a light yellow due to the formation of the ester.5. Distillation:- Set up the distillation apparatus as per the instructor's instructions.- Heat the mixture to about 78°C, which is the boiling point ofethyl acetate.- Collect the distillate in a receiving flask. The distillate should have a fruity odor characteristic of ethyl acetate.6. Analysis:- Use a pH meter to check the pH of the distillate. Ethyl acetate is a neutral compound, so the pH should be close to 7.Results:- The reaction mixture turned a light yellow after the addition of sodium chloride.- The distillation process yielded approximately 5 mL of distillate with a fruity odor.- The pH of the distillate was measured to be 6.8.Discussion:The synthesis of ethyl acetate from ethanol and acetic acid was successful, as evidenced by the formation of a volatile distillate with the characteristic odor of ethyl acetate. The use of concentrated sulfuric acid as a catalyst facilitated the esterification reaction by protonating the carbonyl oxygen of acetic acid, making it more electrophilic and susceptible to nucleophilic attack by the alcohol. The addition of sodium chloride helped to remove water, which could potentially interfere with the reaction by acting as a nucleophile.The distillation process was crucial for isolating the ethyl acetate from the reaction mixture. By carefully controlling the temperature, we were able to collect the desired compound while leaving behind the unreacted starting materials and byproducts.Conclusion:In conclusion, the synthesis of ethyl acetate from ethanol and acetic acid was successfully achieved through the esterification reaction. The use of concentrated sulfuric acid as a catalyst and the distillation process allowed for the isolation of the desired compound. Thisexperiment provided a practical understanding of esterification reactions and the techniques involved in organic synthesis.Appendix:- Chemical Equation:\[ \text{CH}_3\text{CH}_2\text{OH} + \text{CH}_3\text{COOH}\xrightarrow{\text{H}_2\text{SO}_4} \text{CH}_3\text{COOCH}_2\text{CH}_3 + \text{H}_2\text{O} \]- Safety Precautions:- Wear safety goggles and gloves at all times.- Avoid contact with concentrated sulfuric acid and acetic acid.- Do not inhale the vapors of the distillate.。
分析化学实验报告范文(完整版)
报告编号：YT-FS-8612-63分析化学实验报告范文(完整版)After Completing The T ask According To The Original Plan, A Report Will Be Formed T o Reflect The Basic Situation Encountered, Reveal The Existing Problems And Put Forward Future Ideas.互惠互利共同繁荣Mutual Benefit And Common Prosperity分析化学实验报告范文(完整版)备注：该报告书文本主要按照原定计划完成任务后形成报告，并反映遇到的基本情况、实际取得的成功和过程中取得的经验教训、揭露存在的问题以及提出今后设想。
文档可根据实际情况进行修改和使用。
实验题目:草酸中h2c2o4含量的测定实验目的:学习naoh标准溶液的配制、标定及有关仪器的使用;学习碱式滴定管的使用，练习滴定操作。
实验原理:h2c2o4为有机弱酸，其ka1=5、9×10-2，ka2=6、4×10-5、常量组分分析时cka1>10-8，cka2>10-8，ka1/ka2<105，可在水溶液中一次性滴定其两步离解的h+:h2c2o4+2naoh===na2c2o4+2h2o计量点ph值8、4左右，可用酚酞为指示剂。
naoh标准溶液采用间接配制法获得，以邻苯二甲酸氢钾标定:-cook-cooh+naoh===-cook-coona+h2o此反应计量点ph值9、1左右，同样可用酚酞为指示剂。
实验方法:一、naoh标准溶液的配制与标定用台式天平称取naoh1g于100ml烧杯中，加50ml 蒸馏水，搅拌使其溶解。
移入500ml试剂瓶中，再加200ml蒸馏水，摇匀。
准确称取0、4~0、5g邻苯二甲酸氢钾三份，分别置于250ml锥形瓶中，加20~30ml蒸馏水溶解，再加1~2滴0、2%酚酞指示剂，用naoh标准溶液滴定至溶液呈微红色，半分钟不褪色即为终点。
关于英文版化学实验报告
关于英文版化学实验报告篇一：英文版化学实验报告Title: Preparation of Fe scrap from waste(NH4) 2SO4.FeSO4.6H2OThe purpose of the experimentLearn the method used scrap iron preparation of ferrous ammonium sulfate.Familiar with the water bath, filtered, and evaporated under reduced pressure and crystallization basic working.The experimental principle, the iron and sulfuric acid to generate reactive ferrous sulfate, ferrous sulfate and ammonium sulfate in an aqueous solution of equal molar interaction, becomes less soluble blue generate ferrous ammonium sulfate.Fe+H2SO4=FeSO4+H2 (gas)FeSO4+ (NH4)2SO4+6H2O=(NH4)2SO4.FeSO4.6H2O Usually ferrous rocks are easily oxidized in air, but after the formation of relatively stable perfunctory, not to be oxidized.Experiment to use instruments, scales, constant temperature water bath, pumps, basins, cups, 10ml graduated cylinder, asbestos mesh, glass, tripod, alcohol lamp, funnel.Iron pieces to a solid pharmaceutical use, use of acid ammonium sulfate and 3mol / l of sulfuric acid, concentrated sulfuric acid.The experiment was divided into four steps.The first step Said iron powder 4g into a beaker and then 50ml 10ml, 3mol / L H2SO4 was added to the same beaker. The second step will be the beaker is heated to no more bubbles, and then filtered hot and the filtrate was then filled in 100ml beaker. The third step, called 4g (NH4)2SO4, and the resultingammonium sulfate and 5.3ml of water to form a saturated solution, and then add it to the ferrous sulfate solution, adjusted with concentrated sulfuric acid to PH = 1. A fourth step, the third step the solution was heated in a water bath to the surface until the film is crystallized, it was slowly cooled andthen filtered under reduced pressure to stand finally dried, weighed and the yield was calculated. The results obtained 8.1g bluish powdery crystals. Have this result we can calculate yield, starting with the first step we tried to know the amount of iron, should this we can calculate the theoretical sulfate ferrous sulfate is 0.03mol, then ferrous sulfate obtained by the0.03molFeSO4 theoretical value of ammonium. FeSO4+（NH4）2SO4+6H2O=FeSO4.(NH4)2SO4.6H2O 0.03molX molX=0.03molm=XM=0.03molⅹ392g/mol=11.76gYield = the actual value of the formula is divided by the theoreticalvalue by 100%.it will be calculated into the data obtained in a yield of 68.9%.篇二：英文版化学实验报告The preparation of alkali type copper carbonateThe first:the experiment purpose1.Master the methods of alkali type copper carbonate prepared and principle2.Through the design experiment to cultivate independent design ability and chemical research thinkingThe second:the experimental principleThe solubility of Cu(OH)2and CuCO3 are similar, With Cu2(OH)2CO3 solid precipitation in the solution.2CuSO4+2Na2CO3+H2O==Cu2(OH)2CO3↓+2Na2SO4+CO2↑The third:the experimental steps1.Solution preparationDisposes 0.5 mole of each litre acid sour coppers and sodium carbonate solution each 100 milliliters.2.The feeding order and raw material compare the explorationAccording to 2:1.6,2:2,2:2.4,2:2.8 allocated proportion, is accepted after passing an examination the surface disposition acid sour copper and the sodium carbonate solution, joins in separately 8 test tubes, joins rapidly the sulfuric acid copper solutions in the sodium carbonatesolution, vibrates about other constant temperature ten minutes as for 75 degrees Celsius water baths in, the inversion feeding order recreates one time, the observation has the precipitation speed, quantity how many and the color,discovers the optimum condition.3.Temperature explorationAccording to the above optimum condition, takes the acid sour copper solutions and the sodium carbonate solution separately under 50, 75 and 100 degrees Celsius responded that, discovers the optimum temperature.4.According to 2, 3 step exploration optimum condition prepares the final product, and with the distilled water lavation, finally dries and calls heavily.(Enlarges ten times with conical flask to do)The fourth:the experimental itemsInstrument and material: The balance, the beaker, the glass rod, the Volumetric flask, the test tube, the filter flask,the Buchner funnel, the Erlenmeyer flaskChemicals: Copper carbonate, sodium sulfateThe fifth:the experimental result1.By the step 2, the observation phenomenon optimum condition is equal to for the cupric sulfate compared to the sodium carbonate 2:2.4, the feeding order for joins the sulfuric acid copper solutions to thesodium carbonate solution in.2.By the step 3, the observation phenomenon optimum temperature is 75 degrees Celsius3.According to the copper sulfate solution than sodium carbonatesolution is 2:2. 4, ten times magnification, alkali type copper carbonate was zero point five grams, according to the reaction equation calculation yield.2CuSO4+2Na2CO3+H2O==Cu2(OH)2CO3↓+2Na2SO4+CO2↑2 10.5*0.02 X2/(0.5*0.02)=1/XX=0.005M[Cu2(OH)2CO3]=0.005*222=1.11gProductive rate:0.5/1.11*100%=45%The sixth : Questions1. Which cupric salt suit the system to take the cupric basic carbonate? Answer:Cu(NO)3 or CuSO42. The reaction temperature has what influence to this experiment?.Answer:The temperature excessively is low, the response speed is slow; The hyperpyrexia, the Cu2(OH)2CO3 decomposition is CuO.3. Reaction is carried out at what temperature will appear Brownproduct? What is the brown substance?Answer: The temperature is equal to 100 degrees Celsius and this brown material is CuO.篇三：化学专业英语实验报告In the physiological saline the sodium chloride content determinationone, the experimental goal1、the study silver nitrate standard solution configuration and the demarcation method2、the grasping law raises Si Fa to determine the chloride ion the method principle two, the experimental principleWith AgNO3 standard solution titration Cl - Ag + + Cl - = = AgCl，At ph 7.0 -10.5 available fluorescent yellow do indicator (HFIn)HFIn = = FIn (yellow) + H +Sp before: excessive, AgCl precipitation adsorption of Cl - AgCl Cl - + FIn - (yellow-green)After Sp: Ag +, excessive AgCl precipitation Ag + adsorption, adsorption FIn - reprecipitation AgCl, Ag + + FIn - = = AgCl, Ag +, FIn - (pink) The finish color changes: from yellowish green to orange Three, instruments and reagentsEquipment and materials：Acid type buret (150 ml), taper bottle (250 ml), volumetric flask (100 ml), pipette (20 ml, 10 ml), measuringcylinder (100 ml, 10 ml), beaker (100 ml), brown reagent bottles (500 ml), analytical balance, platform scale. The reagent and drug: Analysis of AgNO3 (s, pure), NaCl (s,analysis of pure), physiological saline, fluorescent yellow - starch. Fourth, the experimental stepsAccurately moving 25 ml concentration is 0.7064 mol ╱L of silver nitrate standard solution in the middle of 250 ml volumetric flask, dilute to scale as a standard solution titration.Accurately moving saline 10.00 ml to 250 ml conical flask, add 50 ml water, 3 drops of fluorescent yellow indicator, 5% starch indicator 5 ml, under continuous agitation, using silver nitratestandard solution titration to solution from yellow to pink is the end point. Record the consumption volume of silver nitratestandard solution, parallel determination of 3, calculate the sodium chloride content in saline and relative mean deviation.Fifth, data recording and processingFormula: ρ = V×MrNaCl×CAgNO3 x 100The average deviation d=0.01300 dr=d/ρ×100%=0.13%。
【优质文档】化学英语实验报告-实用word文档 (5页)
本文部分内容来自网络整理，本司不为其真实性负责，如有异议或侵权请及时联系，本司将立即删除！== 本文为word格式，下载后可方便编辑和修改！ ==化学英语实验报告篇一：英文版化学实验报告Preparation of ethyl acetateFirst, the purpose of the experiment:1、 Learn from the general principles of organic synthetic esters and methods2、 Master distillation, extraction, drying and other experimental techniques and its application in aspecific experimentSecond, the experimental principle:Main reaction：CH3COOH+CH3CH2OH=CH3COOCH2CH3+H2OConditions: heating to 120 to 125 °C in concentratedsulfuric acid catalyzedSide effects：浓H2SO4CH3CH2OH--------->CH2=CH2+H2O170度浓H2SO4CH3CH2OH--------->CH3CH2OCH2CH3+H2O140度Third, the instruments and reagents:1、 Instruments and materials: Round-bottomed flask,Spherical condenser, Straight condenser，Distillationhead, a separatory funnel, measuring beakers, dropper, conical flask, thermometer, electric2、 drugs: Glacial acetic acid (AR), absolute ethanol (AR),concentrated sulfuric acid, saturated brine, a saturated sodium carbonate solution, a saturated calcium chloride solution, dried over anhydrous magnesium sulfate, litmusFourth,Reactor：Fifth,Experimental procedure:Adding 50ml round bottom flask 3ml 5ml ethanol and acetic acid, in shaking batch of concentrated sulfuric acid was added1.3ml mixed, and add a few grains of zeolite, and then install the instrument responseLow heat, slowly reflux for 30 minutes. Coolish, reflux device to the distillation apparatus, wetted with cold water to cool the bottle. Heating distillation until the distillate liquid volume is about half the volume of the reaction so far to give the crude product in ethyl acetateThe distillate was slowly saturated sodium carbonate solution was added portionwise, and oscillate until the evolution of carbondioxide gas without using litmus paper test acetate layer was neutral. The mixture was then transferred to a separatory funnel, andseparated aqueous layer was washed once with saturated aqueous saline solution 3ml The organic layer was washed with a saturated solutionof calcium chloride 3ml, washed with water and finally once. The organic layer in a dry Erlenmeyer flask filled with anhydrous magnesium sulfate. The crude ethyl acetate, dried on a water bath heated to distill, collecting fractions 73 to 78°C. Weigh or measure product volume, and calculate the yield point or refractive index measurement products。
化学实验报告_英文
Experiment Title: Determination of the Molar Mass of a Volatile CompoundDate: October 1, 2021Objective:The objective of this experiment is to determine the molar mass of a volatile compound by using the ideal gas law and the known density of the compound.Introduction:The molar mass of a substance is the mass of one mole of that substance. It is an important property used to identify and characterize compounds. In this experiment, we will determine the molar mass of a volatile compound using the ideal gas law and the known density of the compound.Materials:1. Sample of volatile compound2. Graduated cylinder3. Balance4. Beaker5. Thermometer6. Ice bath7. Gas syringe8. Data tableProcedure:1. Measure the mass of the sample using a balance and record the value.2. Pour a known volume of water into a graduated cylinder and record the initial volume.3. Add the sample to the graduated cylinder and record the final volume.4. Calculate the volume of the sample by subtracting the initial volume from the final volume.5. Measure the temperature of the sample using a thermometer and record the value.6. Transfer the sample to a beaker and cool it in an ice bath until the temperature reaches 0°C.7. Use a gas syringe to measure the volume of the gas at 0°C and record the value.8. Calculate the density of the sample by dividing the mass of the sample by the volume of the sample.9. Use the ideal gas law to calculate the molar mass of the compound.Results:1. Mass of the sample: 1.23 g2. Volume of the sample: 2.45 mL3. Temperature of the sample: 25°C4. Volume of the gas at 0°C: 1.20 mL5. Density of the sample: 0.51 g/mLCalculation:1. Molar mass = (mass of the sample / volume of the gas) x (temperature of the gas / pressure of the gas) x (1 atm / 22.4 L/mol)2. Molar mass = (1.23 g / 1.20 mL) x (273.15 K / 298.15 K) x (1 atm / 1.20 mL) x (22.4 L/mol)3. Molar mass = 108.0 g/molDiscussion:In this experiment, we determined the molar mass of a volatile compound by using the ideal gas law and the known density of the compound. Thecalculated molar mass was 108.0 g/mol, which is in good agreement with the literature value of 106.0 g/mol. This indicates that the experimental method used in this experiment is reliable and accurate.Conclusion:The molar mass of the volatile compound was determined to be 108.0 g/mol using the ideal gas law and the known density of the compound. This experiment demonstrates the effectiveness of using the ideal gas law to determine the molar mass of volatile compounds.References:1. Silberberg, M. S. (2012). Chemistry: The Central Science (10th ed.). Boston, MA: McGraw-Hill.2. Atkins, P. W., & de Paula, J. (2014). Atkins' Physical Chemistry(11th ed.). New York, NY: Oxford University Press.。
英文版化学实验报告
Abstract:The objective of this experiment was to prepare iron(III) chloride (FeCl3) by the reaction of iron (Fe) with chlorine gas (Cl2). The experiment aimed to determine the reaction yield and to analyze the purity of the obtained product. The reaction was conducted in a fume hood, and the reaction yield was calculated based on the initial mass of iron and the mass of the resulting iron(III) chloride. The purity of the product was determined by performing qualitative analysis using spectroscopic techniques.Introduction:Iron(III) chloride is a yellowish-green crystalline solid that is widely used in various applications such as dyes, pharmaceuticals, and water treatment. It is also used as a catalyst in organic synthesis. In this experiment, iron(III) chloride was prepared by the reaction of iron with chlorine gas. The balanced chemical equation for the reaction is:2Fe + 3Cl2 → 2FeCl3The reaction is exothermic, and the iron(III) chloride formed is highly reactive and hygroscopic. Therefore, it is crucial to perform the experiment in a controlled environment and handle the chemicals with appropriate safety measures.Materials:1. Iron (Fe) metal2. Chlorine gas (Cl2)3. Fume hood4. Crucible5. Tongs6. Weighing balance7. Spectrophotometer8. Spectroscopic standards for iron(III) chlorideProcedure:1. Weigh the iron metal accurately using a weighing balance and transfer it to a crucible.2. Place the crucible in a fume hood and ensure that the hood is functioning properly.3. Gradually introduce chlorine gas into the fume hood, ensuring that the flow rate is controlled.4. Use tongs to hold the crucible and heat it gently using a Bunsen burner until the iron metal starts to react with the chlorine gas.5. Observe the reaction, which will be indicated by the formation of a reddish-brown smoke and the evolution of heat.6. Continue heating the reaction mixture until no further reaction is observed, and the crucible starts to cool down.7. Allow the crucible to cool to room temperature in the fume hood.8. Transfer the solid product to a clean crucible and weigh it using a weighing balance.9. Calculate the reaction yield by subtracting the initial mass of iron from the mass of the resulting iron(III) chloride.10. Perform qualitative analysis using a spectroscopic technique to determine the purity of the obtained iron(III) chloride.Results:The initial mass of the iron metal used was 0.873 g, and the mass of the resulting iron(III) chloride was 1.347 g. Therefore, the reaction yield was calculated as follows:Reaction yield = (mass of iron(III) chloride / initial mass of iron) × 100%Reaction yield = (1.347 g / 0.873 g) × 100% = 154.7%The purity of the obtained iron(III) chloride was determined by comparing the absorbance of the sample with the absorbance of spectroscopic standards. The calculated purity was found to be 98.5%.Discussion:The experiment was successful in preparing iron(III) chloride from iron and chlorine gas. The reaction yield of 154.7% indicates that the reaction was highly exothermic, and the iron metal was completely consumed in the reaction. However, the reaction yield is slightly higher than the theoretical yield, which may be due to the incompleteconversion of iron to iron(III) chloride or the formation of impurities during the reaction.The purity of the obtained iron(III) chloride was determined to be 98.5%, which is considered to be a good purity level for this compound. The qualitative analysis using spectroscopic techniques confirmed the presence of iron(III) chloride in the product.Conclusion:In conclusion, the experiment successfully prepared iron(III) chlorideby the reaction of iron with chlorine gas. The reaction yield and purity of the obtained product were determined, and the results were within acceptable limits. The experiment provided valuable insights into the reaction kinetics and purity analysis techniques.。
英文版的化学实验报告
Experiment Title: Synthesis of Ethyl AcetateObjective:The objective of this experiment is to synthesize ethyl acetate, an important ester used in various applications such as perfumes, flavors, and solvents. The reaction involves the esterification of acetic acid and ethanol in the presence of an acid catalyst.Experimental Procedure:1. Materials:- Acetic acid (CH3COOH)- Ethanol (C2H5OH)- Concentrated sulfuric acid (H2SO4)- Sodium chloride (NaCl)- Ice- Sodium bicarbonate (NaHCO3)- Ethyl acetate (product)- Distilled water- Erlenmeyer flask (100 mL)- Conical flask (500 mL)- Round-bottom flask (1000 mL)- Distillation apparatus- Heat source- Stirring rod- Thermometer- pH meter- Safety goggles- Lab coat- Gloves2. Procedure:a. Weigh 10.0 g of acetic acid and 5.0 g of ethanol using an analytical balance and transfer them into an Erlenmeyer flask.b. Add 2 mL of concentrated sulfuric acid to the flask and mix the contents thoroughly using a stirring rod.c. Place the flask in an ice bath to maintain a low temperature throughout the reaction.d. After 1 hour, remove the flask from the ice bath and observe the formation of a cloudy solution.e. Add 10 g of sodium chloride to the flask and mix well.f. Slowly add 50 mL of distilled water to the flask while stirring continuously to dilute the solution.g. Transfer the solution to a conical flask and add 10 g of sodium bicarbonate.h. Stir the solution until the acid is neutralized, as indicated by the disappearance of effervescence.i. Set up the distillation apparatus, ensuring that the distillation flask is connected to the condenser and the receiver.j. Heat the mixture slowl y and maintain a temperature between 70°C and 80°C.k. Collect the distillate in the receiver and observe the formation of ethyl acetate.l. Stop the distillation when the temperature rises above 80°C.m. Remove the receiver and allow the ethyl acetate to cool to room temperature.n. Filter the distillate through a filter paper to remove any impurities.Results:1. The reaction mixture was cloudy after 1 hour of reaction, indicating the formation of ethyl acetate.2. The addition of sodium bicarbonate neutralized the acid, causing the disappearance of effervescence.3. The distillation process yielded approximately 10 mL of ethyl acetate, as observed in the receiver.4. The pH of the reaction mixture before neutralization was 2.5, indicating the presence of excess acid.5. The pH of the neutralized mixture was 7, indicating complete neutralization.Discussion:The synthesis of ethyl acetate involves the esterification reaction between acetic acid and ethanol in the presence of an acid catalyst. The reaction proceeds via the formation of an intermediate, the acetyl ethoxide, which then reacts with water to produce ethyl acetate andacetic acid. The addition of concentrated sulfuric acid serves as a catalyst to facilitate the reaction.The formation of a cloudy solution after 1 hour of reaction suggests the successful formation of ethyl acetate. The addition of sodiumbicarbonate neutralizes the excess acid, allowing the ethyl acetate tobe isolated as a distillate. The distillation process is essential for separating the ethyl acetate from the remaining impurities and water.The yield of ethyl acetate obtained in this experiment is approximately 10 mL, which is consistent with the expected yield based on the stoichiometry of the reaction. The reaction conditions, such astemperature and reaction time, play a crucial role in achieving the desired yield and purity of the product.Conclusion:In this experiment, the synthesis of ethyl acetate was successfully achieved through the esterification reaction of acetic acid and ethanol in the presence of an acid catalyst. The reaction mixture was neutralized using sodium bicarbonate, and the ethyl acetate was isolated by distillation. The yield of ethyl acetate obtained was consistent with the expected yield, and the reaction conditions were optimized to achieve the desired results.References:- Advanced Organic Chemistry: Reactions, Mechanisms, and Structure by Francis A. Carey and Richard J. Sundberg- Organic Chemistry by Jonathan Clayden, Nick Greeves, Stuart Warren, and Peter Wothers。
化学实验报告英语作文(3篇)
第1篇Experiment Name: Preparation of Sodium Chloride from SaltwaterDate: [Date]Objective: The objective of this experiment was to prepare sodium chloride from saltwater by the process of evaporation and crystallization.Introduction:Saltwater is a mixture of water and sodium chloride (NaCl), which is commonly found in oceans, seas, and lakes. The concentration of sodium chloride in saltwater can vary, but it is typically around 3.5% by weight. The process of evaporation and crystallization is used to separate sodium chloride from saltwater and obtain pure sodium chloride crystals.Materials:- Saltwater- Evaporating dish- Bunsen burner- Glass stirring rod- Weighing balance- Filter paper- Funnel- Beaker- Test tube- Microscope- Sodium chloride crystals (for comparison)Procedure:1. Measure 100 mL of saltwater using a graduated cylinder and transfer it to an evaporating dish.2. Place the evaporating dish on a hot plate and heat it using a Bunsen burner. Stir the saltwater continuously with a glass stirring rod to prevent localized boiling and ensure even evaporation.3. Observe the evaporation process until the saltwater is reduced to a small volume, approximately 20 mL. At this point, the concentration of sodium chloride has increased significantly.4. Remove the evaporating dish from the hot plate and allow it to cool down to room temperature.5. Once the evaporating dish is cool, observe the crystallization process. Sodium chloride crystals will start to form as the solution cools down.6. Use a filter paper and funnel to collect the sodium chloride crystals from the evaporating dish. Wash the crystals with distilled water to remove any impurities.7. Transfer the sodium chloride crystals to a beaker and dry them usinga Bunsen burner. Allow the crystals to cool down to room temperature before weighing them.8. Compare the weight of the sodium chloride crystals obtained from the experiment with the known weight of sodium chloride crystals (for comparison).Results:- Initial weight of the sodium chloride crystals: [Weight]- Weight of the sodium chloride crystals obtained from the experiment: [Weight]- Known weight of sodium chloride crystals (for comparison): [Weight]Discussion:In this experiment, we successfully prepared sodium chloride from saltwater using the process of evaporation and crystallization. As the saltwater was heated, the water evaporated, leaving behind the sodium chloride crystals. The concentration of sodium chloride in the saltwater increased as the water evaporated, leading to the formation of crystals. The purity of the sodium chloride crystals was determined by comparing the weight of the obtained crystals with the known weight of sodium chloride crystals.The experiment demonstrated the effectiveness of the evaporation and crystallization process in separating sodium chloride from saltwater. However, it is important to note that the purity of the obtained sodium chloride crystals can be affected by various factors such as impurities in the saltwater and the conditions of evaporation and crystallization.Conclusion:The objective of this experiment was achieved by successfully preparing sodium chloride from saltwater using the process of evaporation and crystallization. The obtained sodium chloride crystals were compared with the known weight of sodium chloride crystals, and the experiment was found to be successful in obtaining pure sodium chloride. Further optimization of the experimental conditions could potentially improve the purity of the obtained sodium chloride crystals.第2篇Experiment Title: Synthesis of Ethanol from EtheneDate: October 15, 2023Objective: The objective of this experiment was to synthesize ethanol from ethene using the hydration reaction. The experiment aimed to demonstrate the principles of chemical reactions, the use of laboratory equipment, and the application of safety protocols.Materials:- Ethene (C2H4)- Concentrated sulfuric acid (H2SO4)- Water (H2O)- Sodium chloride (NaCl) solution- Potassium dichromate (K2Cr2O7) solution- Iron (III) chloride (FeCl3) solution- Ethanol (C2H5OH) standard solution- Chloroform (CHCl3)- Distillation apparatus- Gas burner- Test tubes- Beakers- Pipettes- Thermometer- Stirring rod- Safety goggles- Lab coat- GlovesProcedure:1. Preparation of Ethene Solution:- Ethene was passed through a column filled with sodium chloride solution to remove impurities.- The purified ethene was collected in a test tube.2. Hydration Reaction:- A beaker containing concentrated sulfuric acid was heated gently.- The ethene was then passed through the hot sulfuric acid, where it underwent hydration to form ethanol.- The resulting solution was allowed to cool.3. Purification of Ethanol:- The mixture was separated using a separating funnel to remove unreacted ethene and sulfuric acid.- The organic layer, containing ethanol, was collected in a clean beaker.4. Confirmation of Ethanol Formation:- A small amount of the organic layer was mixed with potassium dichromate and iron (III) chloride solutions.- A color change indicated the presence of alcohol, confirming the formation of ethanol.5. Distillation:- The organic layer was transferred to a distillation apparatus.- Ethanol, with a boiling point of 78.37°C, was distilled off a nd collected in a receiver.6. Analysis:- The purity of the distilled ethanol was determined using a gas chromatograph.- The yield of ethanol was calculated based on the initial amount of ethene used.Results:- Ethanol Formation:- The reaction mixture turned yellow upon addition of potassium dichromate and iron (III) chloride, indicating the presence of alcohol.- Distillation:- The distillation process yielded approximately 50 mL of ethanol, corresponding to a yield of 40%.- Gas Chromatography:- The gas chromatography analysis confirmed the purity of the ethanol to be 95%.Discussion:The experiment successfully synthesized ethanol from ethene through the hydration reaction. The use of concentrated sulfuric acid as a catalyst facilitated the reaction, and the distillation process allowed for the separation of pure ethanol. The yield of 40% was reasonable, considering the limitations of the experimental setup and the potential for side reactions. The purity of the ethanol, as determined by gas chromatography, was satisfactory, indicating a successful synthesis.Conclusion:This experiment provided a practical demonstration of the hydration reaction and the synthesis of ethanol from ethene. The use of laboratory techniques and safety protocols was crucial in ensuring the success of the experiment. The results indicate that the synthesis of ethanol is a feasible process, and further optimization could potentially increase the yield and purity of the product.Safety Precautions:- All chemicals were handled with care, and appropriate personal protective equipment, including safety goggles, lab coat, and gloves, was worn at all times.- Concentrated sulfuric acid and other hazardous chemicals were handled using proper techniques to avoid spills and inhalation of vapors.- The gas burner was used with caution, and the distillation apparatus was securely fastened to prevent any accidents.References:- Smith, J. M. (2020). Introduction to Organic Chemistry. New York: Oxford University Press.- Johnson, R. L. (2019). Principles of Chemical Engineering. Boston: McGraw-Hill Education.第3篇Experiment Title: Synthesis of Silver NitrateDate: [Date]Time: [Time]Lab Section: [Lab Section]Lab Partner: [Partner's Name]Abstract:The objective of this experiment was to synthesize silver nitrate by reacting silver with concentrated nitric acid. The experiment aimed to understand the chemical reaction involved, the properties of the products, and the safety precautions associated with the use of hazardous chemicals.Introduction:Silver nitrate is a compound with the chemical formula AgNO3. It is a white crystalline solid that is highly soluble in water. Silver nitrate is used in various applications, including photography, medicine, and the preparation of other silver compounds. In this experiment, we synthesized silver nitrate by reacting silver with concentrated nitric acid.Materials:- Silver metal (shiny silver coins or pellets)- Concentrated nitric acid (HNO3)- Distilled water- Test tubes- Beakers- Glass rods- Safety goggles- Lab coat- Gloves- Bunsen burner- Heat sourceProcedure:1. Wear safety goggles, lab coat, and gloves to ensure personal safety.2. Measure 2-3 silver coins or pellets and place them in a test tube.3. Add 2-3 mL of concentrated nitric acid to the test tube containing the silver.4. Observe the reaction. The silver will react with the nitric acid to form a brown gas (NO2) and a white precipitate (silver nitrate).5. Continue adding concentrated nitric acid to the reaction mixture until the precipitate stops forming.6. Allow the reaction mixture to cool to room temperature.7. Once cooled, carefully add 10 mL of distilled water to the test tube.8. Stir the solution with a glass rod to dissolve the silver nitrate.9. Transfer the solution to a beaker and heat it gently over a Bunsen burner to remove any remaining nitric acid fumes.10. Once the fumes have dissipated, allow the solution to cool to room temperature.11. Transfer the solution to a clean, labeled container for storage.Results:The reaction between silver and concentrated nitric acid produced a white precipitate, which was identified as silver nitrate. The solution turned light brown due to the formation of nitrogen dioxide gas (NO2). The precipitate was observed to be insoluble in water.Discussion:In this experiment, the reaction between silver and concentrated nitric acid was a single displacement reaction. The silver atoms replaced the hydrogen atoms in the nitric acid, forming silver nitrate and nitrogen dioxide gas. The balanced chemical equation for the reaction is:2Ag(s) + 4HNO3(aq) → 2AgNO3(aq) + 2NO2(g) + 2H2O(l)The white precipitate observed was silver nitrate, which is a sparingly soluble salt. The light brown color of the solution was due to the formation of nitrogen dioxide gas, which is a colorless gas under normal conditions but turns brown when dissolved in water.Conclusion:The experiment successfully synthesized silver nitrate by reactingsilver with concentrated nitric acid. The reaction produced a white precipitate, which was identified as silver nitrate. The experiment demonstrated the principles of single displacement reactions and the properties of silver nitrate. It also emphasized the importance of safety precautions when handling hazardous chemicals.References:1. Chang, R. (2016). Chemistry. 13th ed. New York, NY: McGraw-Hill Education.2. Silberberg, M. S. (2016). Chemistry: The Central Science. 14th ed. New York, NY: McGraw-Hill Education.。
英文版化学实验报告(最新整理)
Preparation of n -bromobutane一、Purpose1、Study the principle and method of preparing n-butyl bromide from n-butyl alcohol by treatment with sodium bromide and concentrated sulfuric acid2、Learn the technique of reflux with a gas trap apparatus and washing.二、Principlen-Butyl bromide can be easily prepared by allowing n-butyl alcohto react with sodium bromide and concentrated sulfuric acid.Main reactions ：NaBr + H 2SO4 → HBr + NaHSO424H SO 322232222CH CH CH CH OH HBr CH CH CH CH Br H O+−−−→+Secondary reactions ：；24H SO 32223222CH CH CH CH OH CH CH CH=CH H O−−−→+()24H SO 32223222222CH CH CH CH OH CH CH CH CH O H O−−−→+24222H SO HBr Br SO H O+−−→++三、Materials n-butyl alcohol ：4mL Sodium bromide ：5gConcentrated sulfuric acid ：2.5mL/6mL Anhydrous calcium chloride:0.5g 10% aqueous sodium hydroxide:5mL四、Primary reagent And Product physical constantsNameRelativemolecularmassCharacter RelativedensityMeltingpointBoilingpointRefractiveindexn-bromobutane137.03colorless andtransparentliquid1.299-122.4101.6 1.4399n-butyl alcohol74.12colorless andtransparentliquid0.8098-89.2117.7 1.3993五、Apparatus六、Procedure（1）50mLboiling flask+50mLwater+6mLconcentrated sulfuric acid Cool down（2）Assembling equipment(3) Stop and simple distill(4)(5)七、Experimental records(1) Sulfuric acid soluble in water gives off a lot of heat(2) The solution of the distillation flask become yellow and the sodium bromide dissolve(3)Solution is divided into two layers and liquid of the distillation become clear(4) Liquid layer, upper as the water phase, the lower is positive bromobutane and liquid for the milky haze(5) Liquid at 99 ℃ and stable distillation, after rising to 103 ℃, 103 ℃after fractions and the former part of the don't mix.八、Data recordingOutput:1.3g theoretical yield:5.8g productivity:21.7% Character: colorless and transparent liquid Refractive index:1.4372九、Experiment Discussion1、Turbidity is because it contains a variety of organic phase to organicimpurities2、Plus the bottle stopper of calcium chloride anhydrous dry battery inorder to prevent the water vapor in the air into the conical flask, at the same time prevent product turbidity。
简单的实验报告英语作文
简单的实验报告英语作文Experimental Report: The Effect of Temperature on the Rate of Enzyme Activity。
Introduction。
Enzymes are proteins that catalyze biochemicalreactions in living organisms. They play a crucial role in many biological processes, such as digestion, metabolism, and cellular respiration. Enzyme activity is affected by various factors, including temperature, pH, substrate concentration, and enzyme concentration. In this experiment, we investigated the effect of temperature on the rate of enzyme activity using the enzyme lactase and the substrate lactose.Materials and Methods。
Materials:Lactase solution。
Lactose solution。
Test tubes。
Thermometer。
Water bath。
Timer。
Spectrophotometer。
Methods:1. Prepare lactase solution by diluting 1 mL of lactase stock solution with 9 mL of distilled water.2. Prepare lactose solution by dissolving 1 g of lactose in 100 mL of distilled water.3. Label six test tubes as follows: 0°C, 20°C, 30°C, 40°C, 50°C, and 60°C.4. Add 2 mL of lactase solution to each test tube.5. Place the test tubes in a water bath at the designated temperature for 5 minutes to equilibrate.6. Add 2 mL of lactose solution to each test tube and start the timer.7. Mix the contents of each test tube by gently swirling.8. After 1 minute, remove 1 mL of the reaction mixture from each test tube and transfer it to a spectrophotometer cuvette.9. Measure the absorbance of each sample at 540 nm using a spectrophotometer.10. Repeat steps 8-9 every minute for 5 minutes.11. Record the absorbance values in a table and calculate the average rate of enzyme activity for each temperature.Results。
英文版弗兰克赫兹实验报告
Franck-Hertz ExperimentPurposes1. Measure the first excitation potential of argon atom, and prove the existence ofatom s energy level, thereby strengthen the understanding of energy quantization.2. Learn the microcosmic graphic of the energy exchange which occurs with thecollision of electron and atom, and then explore the main physical factors influencing the process.3. Excise to operate oscilloscope skillfully. EquipmentFranck-Hertz experiment instrument, digital oscilloscope. PrincipleAtom in normal state can neitherradiate nor absorb energy, which is in astable state called stationary state. The energy value to which a certain stationary state corresponds is energy level. The stationary state corresponding to the lowest energy level is called ground state, and others are named excited states.Atom only can jump from one certain energy level to another if its energy changes.Normally, the change of atom stationary state occurs in two situations. The first isU G2KU G2A图 1 夫兰克—赫兹实验I AU G1KA G 2 G 1 KFFigure 1when atom absorbs or radiates energy. The second is when atom is collided by other grains with energy exchange. In order to make atom jump from low energy level to a higher one, this experiment is carried out making an electron run into atom exchanging energy.We can assume that an electronwhich has no initial velocity obtain energy equaling to e*U in an accelerating field. When this electroncollides with atoms in thin argon gas, the energy exchange would happen. Figure 1 shows the schematic diagram of whichcore part is a tetrode filled with argon gas, and electron can be emitted from hot cathode "K ". The main effect of the first grid is to prevent space charge to influence the emission of electron. Accelerating field between anode K and the second grid G 2 can accelerate electron. There is rejection electric field between "A" and "G 2". Figure2 shows the distribution of the potential in the tetrode. If a electron with plenty of energy (more than e *U G2A ) runs into space between "G 2" and "A" through space between "K" and "G 2" , it wouldpush through the rejection field arriving at anode, which can form current thatFigure 2U/VX/cmU G2K /VFigure 3can be detected by galvanometer (GALV). But if a electron loses energy because of colliding with atoms and making them jumping in space "K G2" , the electron wouldn't have enough energy to get over the rejection field, in final, it cannot arrive at the anode, at this time, current go through GALV will decline notably.Observing data showed on GALV carefully while improving the voltage of "U G2K" slowly. If the atom energy level really exist and there is a certain difference between ground state and the first excited state, we can see a section of curve as same as that showed in figure 3.The curve in figure 3 reflects situation of the energy exchange between electron and atoms in space "K G2". Electron in "K G2" would have more and more energy when the voltage in "K G2" increase gradually. At initial stage, electron has a little energy because of a low voltage so that the energy exchange is slight even if it collides with atoms (elastic impact) . Electron going through the second grid would form current "I A " which will increase following the growing of voltage of the second grid "U G2K"(showed by curve "oa" in figure 3). When the voltage in "K G2" equals to the atom's first excitation potential, the electron would collide with atom near the second grid and give all energy obtaining in accelerating field to the atom, which makes the atom jump from ground state to the first excited state. Meanwhile, the electron cannot get over the rejection field and will return to the second grid since it give all its energy to atom. So the anode current decline notably (showed by curve "ab " in figure 3) . Next, electron will have more and more energy following to the increase of voltage of the second grid, so that after a first collision it still has enough energy getting over therejection field to arrive at the anode. Therefore the current go up again, which will not continue until the voltage between K G2is twice the amount of the first excitation potential of atom. It’s electron’s twice collision with atoms that result in the decline of current.(showed by curve “cd”in figure 3). So we can conclusion that as long as in the condition of “U G2K= n* U0（n=1,2,3...）”,the anode current must decline and there will be a curve rising and falling regular which reflects the change of anode current.As showed by the curve, the anode current would not decline suddenly, instead, there is a process of current change. The reason is that the electrons emitted by cathode have different initial velocity(they are not different too much). Otherwise, while most electrons collide with atoms, there are still some electrons arrive at the anode directly without collision, so the anode current will not decline to zero.StepsAbove all, learn the frame of experiment instrument and drill how to use it, next, join the electric wire basing on the requirement of this experiment, at last, switch on the instrument after a careful inspection. The following are some relevant settings: U G1K(between anode and the first grid)=1.3V, U G2K(rejection electric field)=7.5V(1) Choose "manual operation " gears, record data of I A and U G2K while improve the value of U G2K slowly, so that can we calculate the first exciting ( ), and compare that result with the theoretical value(11.5V). Finally, figure out the relatively percentage error.(2)Choose "auto" gears. Measure the first excitation potential of argon atom through observing the curve on digital oscilloscope.Data s dealingFollowing is the data of voltage.n 1 2 3 4 5 6V oltage（V）24.0 35.0 46.5 59.0 72.0 84.0 Calculate the first excitation potential V0.V0=(84-46.5+72-35+59-24)/(3×3)=11.72VCalculate the relatively percentage error.V r=| V0r -V0i |/ V0r *100%=1.93%Result analysisThe relatively percentage error is not too much. The possible reasons for the error are listed as following. 1. We only measure six groups of data, this is not enough.2. The data always changed quickly while we read the data, this would result in errors.。
酵母,实验报告,英文版
Effect of Type of Sugar on Glycolysis and Fermentation in YeastIntroduction:Many cells go through glycolysis and fermentation to break glucose down to carbon dioxide and ethanol (Black et al. 158 and 172). In glycolysis, glucose is converted to pyruvate, and in fermentation, pyruvate is converted to carbon dioxide and ethanol (Black et al. 158 and 172). Glycolysis and fermentation provide these cells, such as yeast, in this experiment, with energy (Peck). However, yeasts do not utilize all kinds of sugar in the same rate. Some sugars can even not be utilized by yeasts (Peck).This experiment aimed to study whether certain types of sugars can be utilized by yeast, if so, what is the different rate that the yeast utilize them. The rate was studied by measuring the rate that the systems produced carbon dioxide, one of final products of fermentation. The sugars being investigated were fructose, galactose, sucrose, maltose, and sactose. Rate that yeast utilized different sugars were compared with the rate that the yeast utilized glucose. The group of yeasts treated with glucose was positive control and that of yeast not treated by any sugar was negative control.In glycolysis, glucose is turned to fructose-6-phosphate, which is the phosphorylated form of glucose (Black et al. 159). Therefore, we expected that yeast would utilize fructose in similar rate as it utilizes glucose. Galactose is a geometric isomer glucose, which is not involved in the process of glycolysis. Hence we hypothesized that galactose cannot be utilized by yeast. Since each disaccharide molecule contains two subunits of monosaccharide monomers, yeast should decompose disaccharides into monosaccharides before going through glycolysis. Therefore, wehypothesized that yeast would utilize disaccharides in slower rate than it would utilize monosaccharides due to one more process that it needs in the overall process. Among disaccharides, the yeast would decompose sucrose and maltose in identical rates since the former is composed of glucose monomer and fructose monomer and the latter one is composed of two glucose monomer. We also hypothesized that yeast would decompose lactose in a slower rate since we expected that galactose, one of its two monomers, cannot be utilized in glycolysis.Materials and Methods:In this experiment, we studied the types of sugars that yeasts can utilize and the differences in rate that yeasts utilize sugars by applying fructose, galactose, sucrose, maltose, and lactose to five groups of yeast respectively. The positive control was set as the group of yeast that was treated with glucose and the negative control was set as the group of yeast that was only treated with buffer and pure water (Peck). Because carbon dioxide was a final product of the overall reaction, amount of carbon dioxide produced was proportional to the amount of sugar being consumed. Therefore, the rates that yeasts utilized sugars were indicated by amount of carbon dioxide being produced in a certain time period. We measured the amount of carbon dioxide produced by using a respirometer. The increase in volume of gas bubble in the respirometer indicated the volume of carbon dioxide produced. The rate that yeast utilized sugars were calculated by dividing volume of carbon dioxide produced (in milliliter) by time (in hour). This value was positively proportional to the rate that yeast utilized the sugar. We avoided radical change in pH value during the experiment by adding some kind of buffer solutions into all test tubes (Peck).Results:Figure 1: The relationship between the rates that yeasts utilized sugars and type of sugars added to yeasts. The rate is determined by change in volume of the bubble in respirometer divided by time that yeast contacted with sugar. The group that treated with yeast was the positive control in this experiment. The error bars represents standard errors.The rates that yeasts utilized fructose and sucrose were statistically identical to the rate that it utilized glucose, because the differences in rates were less than one standard error (figure 1). The rate that yeast utilized maltose was a half of the rate that it utilized glucose. The changes in volume of gas bubble in respirometers of the group of lactose and galactose are statistically same to the change in negative control.Discussion:The yeasts could go through fermentation process with fructose, sucrose, and maltose, but could not go through fermentation with galactose and lactose, because the changes in volume of respirometer in groups treated with galactose and lactose were statistically same to change involume of the negative control group, in which no fermentation would happen because no sugars were added. However, the rate that yeast utilized maltose was half of the rate that it utilized glucose.The hypothesis about monosaccharides was proved to be correct because the yeast could not utilize galactose and utilized glucose and fructose in the same rate. But the experimental results regarding yeast utilization of disaccharides were different from the hypothesis because sucrose, which was expected to be utilized more slowly than monosaccharides, was utilized in the same rate as glucose was, and the yeast was not able to utilize lactose. We can conclude that yeast can utilize fructose, glucose, and sucrose in the same rate and utilize maltose at a half rate than it utilized the former sugars. It cannot undergo fermentation with galactose and lactose. The differences between result and hypothesis suggest that there are other factors determining if yeast can utilize sugars and the rate that yeast utilize them.Since glycolysis is a process in which glucose is turned into pyruvate, the glucose is necessary for glycolysis to happen (Black et al. 158). Therefore, if the yeast doesn’t have enzymes required to convert other kinds of sugars to glucose, glycolysis cannot happen. Since yeast can utilize maltose and sucrose, it must have enzyme that can convert maltose and sucrose into glucose. Similarly, as yeast cannot utilize lactose or galactose, we can deduce that it lacks the enzyme necessary to convert lactose and galactose to glucose. However, fructose is an exception in this experiment. Fructose-6-phosphate, the phoshphyrated form of fructose, is part of glycolysis process (Black et al. 159). Hence the yeast can undergo glycolysis without converting it to glucose. The relatively low rate of utilizing maltose may be caused by low level of enzymes that convert maltose to glucose in yeast. If the yeast converts maltose to glucosemore slowly than it converts sucrose, then the amount of glucose that can undergo glycolysis will be less, and the rate that yeast utilizes maltose will hence be consequently slow.As glycolysis can only take place in cytoplasm, the sugar molecules must first enter the yeast cells (Black et al. 159). Since sugar molecules are polar, they are not likely to enter the cytoplasm through diffusion. Therefore, yeast should have proteins that help transfer certain kind of sugar molecules into its cytoplasm. It is possible that yeast doesn’t have specific type of protein that can help transport galactose and lactose into cytoplasm, and hence cannot undergo the process of glycolysis. The low rate that the yeast utilized maltose might be caused by the low rate that maltose is transported by the specific protein that transports the maltose.Yeast fermentation is a crucial process of making wines and other alcoholic drinks, since ethanol is the ultimate product of this process. Studying the rate of yeast fermentation under different types of sugars can help us find out a more efficient way of producing ethanol. Therefore, results from this experiment may suggest the most efficient type of sugar that we can use to produce wines and other alcoholic drinksAcknowledgement:I would like to thank Professor Peck for helping me set up procedures of the experiment. My partners Maddy and Echo were very helpful during the experiment.Works Cited:1.Peck, Ron. “Glycolysis and Fermentation in Yeast.” Colby College, 2014. Print.2.Black, Michael, Emily Taylor, Jon Monroe, Lizabeth Alliison, Greg Podgorski, andKim Quillin. Biological Science. 5th ed. Glenview: Pearson, 2014. Print.。
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TitleThe title for the lab report may be provided by your lecturer. If not, you will need to make up your title. It should be brief, informative, and interesting. It is not usually a sentence. You should aim to provide just enough information in the title to avoid it being overly general. The key is to be concise and meaningful.Check with your lecturer if you need to include a title page and ensure all the relevant information is supplied. This will include your name, student number, date of the experime nt, the demonstrator’s name and the group you belong to.IntroductionThe introduction should be clear and concise. It should tell the reader what to expect in the report. An introduction generally includes the following elements:• Problem – State the issue investigated by the experiment.•Background –Briefly summarise previous research on the topic and narrow the scope of the study.• Objectives – State the aim of the experiment and state the methods used.• Hypothesis – If this is not already given, you must formulate this in unambiguous terms.The introduction is written in the past tense following the scientific style of writing. Materials and methodsThis section should contain a clear enough explanation of how you conducted the experiment so that someone wishing to replicate the procedure may be able to do so. Here you should describe the experimental design, the treatments and the apparatus you used. You should follow the rules for the conventional descriptions of chemicals. The standard practice is not to use trade names for chemicals. Instead you should use the generic or chemical names. Standard apparatus should be described in proper technical terms. Also, you should describe the procedures and methods of measurement you used. At the end of this section you should provide details of how you analysed the data. If this involved lengthy statistical calculations, these should be attached as an appendix.Results and discussionThis section should be organised in a systematic way such that you first present the results and then discuss them.To report on results you should describe what happened. This is perhaps the most important section of your report because it is where you report the data upon which your conclusions are based. Accuracy, clarity of expression and systematic presentation of the data (e.g., use of tables, graphs, figures, diagrams, etc.) are key factors here. Take note that tables and figures do not simply repeat information given in the text –they are meant to summarise, amplify, or complement it. You should report first the results that bear directly on the title of your lab report. Any other interesting findings should follow this. If the experiment had more than one hypothesis, you may want to organise your results in a way that reflects this. A keyprinciple is never to falsify the results, even if the results did not support a well-accepted hypothesis.Once you have reported the results of the experiment you need to discuss them. This requires analytical thinking to enable you to explain the results. The discussion section should have clear connections with what you said in the introduction and to relevant literature on the topic. You need to say whether or not the results supported the hypothesis. If not, you should provide possible reasons. At this stage you may also comment on issues such as problematic methodology (i.e., design and procedures) or reliability.This section should end with a concluding paragraph (or statement) about the significance of your findings, and where applicable suggest further steps in the scientific process (e.g., that it may be advisable to repeat the experiment with slightly different procedures, or that future researchers could explore a different dimension to the design).ReferencesAll information (i.e. ideas and words) from other sources used in your report must be accurately cited in-text and the full bibliographic information supplied in the reference list at the end. Do not include sources that you have not cited in the reference list. In adopting a particular referencing system, you need to follow the rules consistently throughout your report.Appendices (occasionally)These are not included in all lab reports. They should be used when you need to include detailed information to support/substantiate something you have said in the report. For example, it might include the raw data of your results. If there are several appendices, they need to be numbered with clearly indicated headings. When you make reference within your report to where the reader may find the detailed information, you should refer to the appendix by number (as you would do for tables and figures).Laboratory report checklist• Have you put your name, student number, date of the experiment and the demonstrator’s name on your l ab report?• Were you clear about the hypothesis you were testing?• Have you included all the appropriate sections in your lab report?• Are your charts, figures and graphs drawn in the correct format?• Are all sources correctly in-text and end-text referenced?• Did you hand in your lab report on time and in the correct format?• Did you keep a copy of your report for your own records? AcknowledgementsThis material was modified from source documents prepared by Kuki Singh, ECU, September 2007. Editor: Trevor Bennett.。