关于英文版化学实验报告.doc
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.。
英文版化学实验报告
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 constants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。
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.。
关于化学实验的英文作文
关于化学实验的英文作文英文：Chemistry experiments have always been a fascinating part of my academic journey. The hands-on experience and the thrill of seeing chemical reactions take place right in front of my eyes have always been a source of excitementfor me. One of the most memorable experiments I have conducted was the synthesis of aspirin in the organic chemistry lab.The experiment involved several steps, including the esterification of salicylic acid with acetic anhydride, followed by the hydrolysis of the ester and the isolation of the aspirin product. It was a complex process that required precision and careful attention to detail. I remember being nervous about handling the chemicals and making sure that I followed the procedure correctly.As I mixed the reagents and observed the changes in thereaction mixture, I couldn't help but feel a sense of anticipation. When the aspirin crystals began to form, it was a moment of triumph for me. Seeing the white, powdery crystals at the bottom of the flask was incredibly satisfying, knowing that I had successfully synthesized a common household medication.The experience taught me the importance of following instructions and understanding the principles behind the reactions. It also highlighted the significance of safety measures in the laboratory. I learned to wear protective gear, handle the chemicals with care, and clean up the workspace diligently after the experiment.Overall, the synthesis of aspirin was a valuable learning experience that not only deepened my understanding of organic chemistry but also instilled in me a sense of responsibility when conducting experiments. It was a reminder that chemistry is not just about mixing chemicals in a lab, but about applying knowledge and skills to achieve a desired outcome.中文：化学实验一直是我学术生涯中令人着迷的一部分。
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.。
英文版实验报告
英文版实验报告英文版实验报告Introduction:In this report, we present the findings and analysis from a recent experiment conducted to investigate the effects of caffeine on cognitive performance. Caffeine, a widely consumed psychoactive substance, is known to have stimulant effects on the central nervous system. The objective of this experiment was to examine whether caffeine could enhance cognitive abilities such as attention, memory, and reaction time.Methodology:Participants: A total of 50 healthy adult volunteers aged between 18 and 30 years were recruited for the study. They were randomly assigned to two groups: the experimental group (received caffeine) and the control group (received a placebo).Procedure: Participants arrived at the laboratory after an overnight fast and were instructed to abstain from consuming any caffeinated beverages or food for at least 12 hours prior to the experiment. They were then given either a capsule containing 200mg of caffeine or a placebo capsule. The experimenters, as well as the participants, were blinded to the group assignments.Cognitive tests: After a 30-minute absorption period, participants completed a battery of cognitive tests. These included a sustained attention task, a memory recall task, and a reaction time test. The tests were designed to measuredifferent aspects of cognitive function.Results:The results of the experiment revealed interesting insights into the effects of caffeine on cognitive performance. Participants in the experimental group, who received caffeine, demonstrated significantly better performance on the sustained attention task compared to those in the control group. They also exhibited improved memory recall and faster reaction times.Discussion:The findings of this experiment support the hypothesis that caffeine can enhance cognitive abilities. The stimulant properties of caffeine may have contributed to the improved attention and memory performance observed in the experimental group. The faster reaction times may be attributed to the increased alertness and arousal associated with caffeine consumption.These results are consistent with previous research on the effects of caffeine on cognitive function. Caffeine has been shown to increase alertness, improve attention, and enhance memory in various studies. However, it is important to note that individual responses to caffeine can vary, and some individuals may experience negative effects such as increased anxiety or disrupted sleep. Implications:The findings of this experiment have implications for various fields, including education, workplace productivity, and even sports performance. The use of caffeine as a cognitive enhancer may be beneficial in situations that requiresustained attention and mental alertness, such as during exams or high-pressure tasks.However, it is crucial to consider the potential risks and limitations associated with caffeine consumption. Excessive intake of caffeine can lead to adverse effects such as jitteriness, increased heart rate, and disrupted sleep patterns. Therefore, it is recommended to consume caffeine in moderation and be aware of individual tolerance levels.Conclusion:In conclusion, this experiment provides evidence that caffeine can enhance cognitive performance, particularly in the domains of attention, memory, and reaction time. The findings support the use of caffeine as a cognitive enhancer, but caution should be exercised regarding its potential side effects. Further research is needed to explore the long-term effects of caffeine on cognitive function and to identify optimal dosages for different populations.。
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。
英文实验报告化学
Abstract:The synthesis of nanocrystalline copper phthalocyanine (CuPc) wascarried out using a solvothermal method. The reaction conditions, including the choice of solvent, temperature, and time, were optimized to achieve the highest yield and purity of CuPc. The synthesized CuPc was characterized using various techniques such as UV-Vis spectroscopy, X-ray diffraction (XRD), scanning electron microscopy (SEM), and transmission electron microscopy (TEM). The results indicate that the solvothermal method is an efficient and effective approach for the synthesis of CuPc nanocrystals with high purity and excellent optical properties.1. Introduction:Copper phthalocyanine (CuPc) is a well-known blue pigment with significant applications in various fields, including optoelectronics, catalysis, and medicine. The unique optical and electronic properties of CuPc, such as its strong absorption in the visible region and high thermal stability, make it an attractive material for many applications. In recent years, the development of nanocrystalline CuPc has gained considerable attention due to its enhanced properties compared to its bulk counterpart. The solvothermal method has been widely used for the synthesis of various inorganic and organic nanomaterials due to its simplicity, cost-effectiveness, and environmentally friendly nature.2. Materials and Methods:2.1 Materials:- Copper(II) sulfate pentahydrate (CuSO4·5H2O)- Potassium phthalocyanine (K3Pc)- Sodium hydroxide (NaOH)- Ethanol (EtOH)- Deionized water2.2 Synthesis of CuPc Nanocrystals:The synthesis of CuPc nanocrystals was carried out using the solvothermal method. The detailed procedure is as follows:1. Dissolve 0.5 g of CuSO4·5H2O and 0.5 g of K3Pc in 10 mL of ethanol under magnetic stirring for 1 hour.2. Add 0.5 g of NaOH to the solution and continue stirring for another hour.3. Transfer the reaction mixture into a Teflon-lined autoclave and heat it at 180°C for 12 hours.4. Cool the autoclave to room temperature and centrifuge the reaction mixture at 5000 rpm for 30 minutes.5. Wash the precipitate with ethanol and deionized water several times to remove impurities.6. Dry the precipitate in an oven at 60°C for 12 hours to obtain the final product.2.3 Characterization Techniques:The synthesized CuPc nanocrystals were characterized using the following techniques:- UV-Vis spectroscopy (Shimadzu UV-2600)- X-ray diffraction (XRD) (Bruker D8 Advance)- Scanning electron microscopy (SEM) (Hitachi S-4800)- Transmission electron microscopy (TEM) (JEOL JEM-2100)3. Results and Discussion:3.1 UV-Vis Spectroscopy:The UV-Vis absorption spectrum of the synthesized CuPc nanocrystals is shown in Figure 1. The spectrum exhibits a strong absorption peak at 640 nm, which is characteristic of CuPc. The shoulder peak at 690 nm is attributed to the transition of π-π.Figure 1: UV-Vis absorption spectrum of CuPc nanocrystals3.2 XRD Analysis:The XRD pattern of the synthesized CuPc nanocrystals is shown in Figure 2. The diffraction peaks are well matched with the standard JCPDS card No. 12-0465, indicating the presence of CuPc in the crystalline form. The crystal size of the CuPc nanocrystals was calculated to be approximately 20 nm.Figure 2: XRD pattern of CuPc nanocrystals3.3 SEM Analysis:The SEM image of the synthesized CuPc nanocrystals is shown in Figure 3. The image reveals the spherical shape of the nanocrystals with an average diameter of 20 nm.Figure 3: SEM image of CuPc nanocrystals3.4 TEM Analysis:The TEM image of the synthesized CuPc nanocrystals is shown in Figure 4. The image confirms the spherical shape of the nanocrystals with a size of approximately 20 nm. The high-resolution image shows the crystalline structure of the CuPc nanocrystals.Figure 4: TEM image of CuPc nanocrystals4. Conclusion:In this study, the solvothermal method was employed for the synthesis of nanocrystalline CuPc. The optimized reaction conditions, including the choice of solvent, temperature, and time, resulted in the formation of CuPc nanocrystals with high purity and excellent optical properties. The synthesized CuPc nanocrystals were characterized using various techniques, including UV-Vis spectroscopy, XRD, SEM, and TEM. Theresults indicate that the solvothermal method is an efficient and effective approach for the synthesis of CuPc nanocrystals with high purity and excellent optical properties.5. Acknowledgments:The authors would like to acknowledge the financial support from the National Natural Science Foundation of China (Grant No. 123456) and the China Scholarship Council (Grant No. 789012).References:1. A. G. Aliev, V. I. Gerasimchuk, A. A. Shevchenko, and A. V. Shevchenko, "Preparation and properties of CuPc/CdS core-shell quantum dots," Journal of Nanomaterials, vol. 2012, Article ID 682318, 2012.2. S. M. Y. Y. Ahamed, S. S. Al-Asfour, and A. A. Al-Asfour, "Synthesis and characterization of copper phthalocyanine thin films using chemical bath deposition method," Journal of Nanomaterials, vol. 2013, Article ID 982916, 2013.3. X. J. Wang, Z. Y. Chen, Y. J. Gao, Y. J. Li, and J. P. Zhang, "Preparation and characterization of CuPc nanocrystals using a microwave-assisted solvothermal method," Journal of Nanomaterials, vol. 2013, Article ID 916402, 2013.4. M. A. E. Al-Asfour, S. S. Al-Asfour, and A. G. Aliev, "Preparation and characterization of copper phthalocyanine/CdS core-shell quantum dots using a solvothermal method," Journal of Nanomaterials, vol. 2014, Article ID 382594, 2014.5. M. A. E. Al-Asfour, S. S. Al-Asfour, and A. G. Aliev, "Preparation and characterization of copper phthalocyanine nanocrystals using a microwave-assisted solvothermal method," Journal of Nanomaterials, vol. 2014, Article ID 382594, 2014.。
【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.。
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)The 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) 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 50ml10ml, 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 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 bluish powderycrystals. Have this result we can calculate yield, starting with the first step we tried to know the amount of iron, should this wecan calculate the theoretical sulfate ferrous sulfate is , thenferrous sulfate obtained by thetheoretical value of ammonium. FeSO4+（NH4）2SO4+6H2O=FeSO4.(NH4) molX=m=XM=ⅹ392g/mol=Yield = the actual value of the formula is divided by the theoretical value by 100%.it will be calculated into the dataobtained in a yield of %.篇二：英文版化学实验报告The preparation of alkali type copper carbonateThe first:the experiment purposethe methods of alkali type copper carbonate prepared andprinciplethe design experiment to cultivate independent design abilityand 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 stepspreparationDisposes mole of each litre acid sour coppers and sodiumcarbonate solution each 100 milliliters.feeding order and raw material compare the explorationAccording to 2:,2:2,2:,2: 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 carbonate solution, 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.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.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 resultthe step 2, the observation phenomenon optimum condition is equal to for the cupric sulfate compared to the sodium carbonate 2:, the feeding order for joins the sulfuric acid copper solutions to the sodium carbonate solution in.the step 3, the observation phenomenon optimum temperature is 75 degrees Celsiusto 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 1* X2/(*)=1/XX=M[Cu2(OH)2CO3]=*222=Productive rate:/*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 Brown product? 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 - 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), measuring cylinder (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 co ncentration is 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 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= dr=d/ρ×100%=%实验名称：硅片的清洗实验目的：1.熟悉清洗设备2.掌握清洗流程以及清洗前预准备实验设备：1.半导体兆声清洗机（SFQ-1006T）；SC-2实验背景及原理：清洗的目的在于清除表面污染杂质，包括有机物和无机物。
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。
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。
化学实验报告模板(完整版)
报告编号：YT-FS-8761-61化学实验报告模板(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化学实验报告模板(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。
实验步骤(1) 在试管中加入5mL5%的过氧化氢溶液，把带火星的木条伸入试管;(2) 加热实验(1)的试管，把带火星的木条伸入试管;(3) 在另一支试管中加入5mL5%的过氧化氢溶液，并加入2g二氧化锰，把带火星的木条伸入试管;(4) 待实验(3)的试管内液体不再有现象发生时，重新加热3mL5%的过氧化氢溶液，把带火星的木条伸入试管;(该步骤实验可以反复多次)(5) 实验后将二氧化锰回收、干燥、称量。
实验现象及现象解释：实验编号实验现象现象解释(1) 木条不复燃(2) 木条不复燃 H2O2分解O2速度太慢没足够的O2试木条复燃.(3) 3H2O2产生大量气泡木条复燃 MnO2使H2O2加速分解O2,O2使木条复然(4) 新加入的H2O2产生大量气泡因为MnO2继续作为催化挤的作用!H2O2继续分解(5) 5MnO2的质量不变因为MnO2是催化剂所以只是改变化学反应速度,不改变其化学性质和质量这里填写您企业或者单位的信息Fill In The Information Of Your Enterprise Or Unit Here。
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。
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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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 resulting ammonium 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 powderycrystals. 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 theoretical value 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 carbonate solution, 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 the sodium 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 Brown product? 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 experimentalprincipleWith 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 reagents Equipment and materials：Acid type buret (150 ml), taper bottle (250 ml), volumetric flask (100 ml), pipette (20 ml, 10 ml), measuring cylinder (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%。