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關(guān)于英文版化學(xué)實(shí)驗(yàn)報(bào)告（精選5篇）
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英文版化學(xué)實(shí)驗(yàn)報(bào)告 1
Title: Preparation of Fe scrap from waste
(NH4) 2SO4.FeSO4.6H2O
The purpose of the experiment
Learn 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 and
then 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 the
0.03molFeSO4 theoretical value of ammonium. FeSO4+（NH4）2SO4+6H2O=FeSO4.(NH4)2SO4.6H2O 0.03molX mol
X=0.03mol
m=XM=0.03molⅹ392g/mol=11.76g
Yield = 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%.
英文版化學(xué)實(shí)驗(yàn)報(bào)告 2
The preparation of alkali type copper carbonate
The first:the experiment purpose
1.Master the methods of alkali type copper carbonate prepared and principle
2.Through the design experiment to cultivate independent design ability and chemical research thinking
The second:the experimental principle
The 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 steps
1.Solution preparation
Disposes 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 exploration
According 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 exploration
According 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 items
Instrument and material: The balance, the beaker, the glass rod, the Volumetric flask, the test tube, the filter flask,the Buchner funnel, the Erlenmeyer flask
Chemicals: Copper carbonate, sodium sulfate
The fifth:the experimental result
1.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 Celsius
3.According to the copper sulfate solution than sodium carbonate
solution 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
0.5*0.02 X
2/(0.5*0.02)=1/X
X=0.005
M[Cu2(OH)2CO3]=0.005*222=1.11g
Productive rate:0.5/1.11*100%=45%
The sixth : Questions
1. Which cupric salt suit the system to take the cupric basic carbonate? Answer:Cu(NO)3 or CuSO4
2. 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.
英文版化學(xué)實(shí)驗(yàn)報(bào)告 3
In the physiological saline the sodium chloride content determination
one, the experimental goal
1、 the study silver nitrate standard solution configuration and the demarcation method
2、 the grasping law raises Si Fa to determine the chloride ion the method principle two, the experimental principle
With 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 steps
Accurately 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 nitrate
standard solution titration to solution from yellow to pink is the end point. Record the consumption volume of silver nitrate
standard solution, parallel determination of 3, calculate the sodium chloride content in saline and relative mean deviation.
Fifth, data recording and processing
Formula: ρ = V×MrNaCl×CAgNO3 x 100
The average deviation d=0.01300 dr=d/ρ×100%=0.13%
英文版化學(xué)實(shí)驗(yàn)報(bào)告 4
Abstract:
Provide a brief summary of the experiments purpose, key procedures, major findings, and conclusions. Aim for conciseness while ensuring all essential points are covered.
Introduction:
Background Information: Discuss the context of the experiment, including relevant theories, principles, and the significance of the study.
Purpose Clearly state the objectives of the experiment.
Hypothesis: If applicable, present a hypothesis based on your understanding of the subject matter.
Materials and Methods:
List all materials used, equipment employed, and the step-by-step procedure followed during the experiment. Ensure that the method is described in sufficient detail for others to replicate the experiment.
Materials: List chemicals, reagents, and any other consumables.
Equipment: Mention instruments, apparatus, and their specifications.
Procedure: Outline the experimental steps in chronological order.
Results:
Present the data collected during the experiment in a structured manner. This may include tables, graphs, and/or photographs of experimental setups and observations.
Data Tables: Organize raw data into tables with appropriate headings.
Graphs: Plot significant data trends using graphs to facilitate analysis.
Observations: Describe any qualitative observations made during the experiment.
Discussion:
Interpret your results, comparing them to the hypothesis (if any), literature findings, and expected outcomes. Discuss possible sources of error and how they might have influenced the results.
Analysis of Results: Explain what the results mean in terms of the experimental objectives.
Comparison with Literature: Relate your findings to existing research.
Sources of Error: Identify potential errors and their impacts on the accuracy and reliability of your results.
Suggestions for Improvement: Offer suggestions for refining the experiment or addressing identified issues.
Conclusion:
Summarize the main findings of the experiment, restate its significance, and provide final thoughts on whether the objectives were achieved.
References:
List all sources cited in the report, following a standard citation format (e.g., APA, MLA, or other as required by your institution).
Appendices:
Include any additional information or supporting materials that are not essential for the main body of the report but may be useful for reference, such as detailed protocols, additional data tables, or raw data sheets.
英文版化學(xué)實(shí)驗(yàn)報(bào)告 5
I. Purpose of the Experiment
To learn the general principles and methods of organic synthetic esters.
To master distillation, extraction, drying, and other experimental techniques and their application in a specific experiment.
II. Experimental Principle
Main Reaction: CH3COOH + CH3CH2OH → CH3COOCH2CH3 + H2O
Concentrated H2SO4 + CH3CH2OH → CH2=CH2 + H2O at 170°C
Concentrated H2SO4 + CH3CH2OH → CH3CH2OCH2CH3 + H2O at 140°C
Conditions: Heating to 120-125°C in concentrated sulfuric acid catalyzed.
Side Effects:
III. Instruments and Reagents
Instruments and Materials:
Round-bottomed flask
Spherical condenser
Straight condenser
Distillation head
Separatory funnel
Measuring beakers
Dropper
Conical flask
Thermometer
Electric heater
Drugs:
Glacial acetic acid (AR)
Absolute ethanol (AR)
Concentrated sulfuric acid
Saturated brine
Saturated sodium carbonate solution
Saturated calcium chloride solution
Anhydrous magnesium sulfate for drying
Litmus paper
IV. Reactor Setup
(Reactor setup instructions can be described here if needed, but it’s typically assembling the instruments mentioned above in a specific order for the distillation process.)
V. Experimental Procedure
Add 50 ml of glacial acetic acid and 3 ml of absolute ethanol to a 50 ml round-bottomed flask.
Add 1.3 ml of concentrated sulfuric acid dropwise while shaking the flask gently.
Add a few grains of zeolite (to prevent boiling over).
Assemble the distillation apparatus and heat the flask slowly to initiate reflux for 30 minutes.
Cool the reflux apparatus slightly and then transfer it to the distillation setup. Cool the flask with cold water.
Heat the distillation apparatus until the distillate liquid volume is about half of the original reaction volume. This will give the crude product of ethyl acetate.
Add the distillate slowly to a saturated sodium carbonate solution in portions, and shake until the evolution of carbon dioxide gas stops. Test the acetate layer for neutrality using litmus paper (optional).
Transfer the mixture to a separatory funnel and wash the aqueous layer once with 3 ml of saturated aqueous saline solution.
Wash the organic layer with 3 ml of a saturated solution of calcium chloride, then wash with water once more.
Dry the organic layer in a dry Erlenmeyer flask filled with anhydrous magnesium sulfate.
Distill the crude ethyl acetate on a water bath, collecting fractions at 73-78°C.
Weigh or measure the product volume and calculate the yield or refractive index.
VI. Discussion
Question: Can a concentrated sodium hydroxide solution be used in place of a saturated sodium carbonate solution for washing the distillate?
Answer: No. A strong base like sodium hydroxide would cause the hydrolysis of ethyl acetate, thereby reducing the yield.
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