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chemical reaction lab report on chemical reactions
chemical reaction lab report on chemical reactions
chemistry chemical reactions lab report
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The experiment was to investigate what are the products of a chemical reaction, more specifically, what iron compound is formed. A chemical reaction is anything that has had a color change, the formation of a solid, bubble, or a temperature change. In an oxidation-reduction reaction, charges of molecules are going to change. The first balanced equation was Cu〖SO〗_4+Fe(s)→Fe〖SO〗_4+Cu. The second balanced equation was 2Cu〖SO〗_4+3Fe(s) →3〖Fe〗_2 (〖SO〗_4 )_3+Cu. Given the two different chemical formulas, the theoretical yield was found to determine how much copper would be left over after the reaction by using the balanced chemical equations and stoichiometry. With the iron being the limiting reagent, we knew that the excess of copper product …show more content…
After figuring out the mass of the empty beaker to be 72.5 grams, 100 milliliters of water were heated using a hot plate. The water warmed just below boiling. Once the beaker of water was removed from the hot plate, 12.1 grams of copper (II) sulfate was added. Once the copper (II) sulfate was stirred, 1.5 grams of iron filling was added to the beaker and set to allow the copper to settle on the bottom of the beaker. Once the beaker was cool enough to touch and the copper was settled to the bottom, we began the decanting process. Decanting was used to remove the limiting reagent, the iron sulfate compound, to dry out the excess reagent, the copper. The copper was decanted twice again with water to clean off any left over iron sulfate compound. Then the copper was covered with acetone and put in an oven for 15 minutes to dry completely. Once the copper was dried, the electronic balance was used again to measure the mass of the beaker and the copper. Once this mass was calculated to be 75.2 grams, the empty beaker’s mass of 72.5 grams was subtracted from it to give us the total mass of the copper, which was 2.68 grams. We knew a reaction occurred when a solid formed at the bottom of the …show more content…
This answer of 104% is our percent yield. With our percent yield being over 100%, human errors obviously occurred. The mass of the beaker could be off or if more than 1.5 grams of the iron filling was added, this can answer the reasoning for having more than 100% percent yield. Our group still managed to say that the product formed was iron (III) sulfate. When comparing data with other groups, there was a vast range of percent yields in the lab. Possible error with decanting or not allowing the copper to completely dry could have answered the fluctuation in numbers. Our group was the only one a percent yield of over 100% but still had the correct iron filling. When checking over the calculations, the class agreed that the product produced was iron (III) sulfate. After checking our calculations again, there is no answer for how our group had over 100% percent yield, even with decanting. Usually during decanting, it is usually not as
Experiment: First prepared a well plate with the appropriate amounts of distilled water, HCl, and Na2S2O3 in each well according to the lab manual. The well where the reaction
The objective of this lab was to calculate the ratio of the copper sulfur compound to conclude whether the compound is made of copper I or II.
The purpose of this lab was to to cycle solid copper through a series of chemical forms and return it to its original form. A specific quantity of copper undergo many types of reactions and went through its whole cycle, then returned to its solid copper to be weighted. We observed 5 chemical reactions involving copper which are: Redox reaction (which includes all chemical reactions in which atoms have their oxidation state changed), double displacement reaction, precipitation reaction, decomposition reaction, and single displacement reaction.
The percent error or percent yield between the theoretical yield of Cu produced and experimental value of Cu produced was approximately 107 %. One source of error, which was a scientific error, was that leaving the Cu precipitate in the cupboard for week allows dust to accumulate on the sample. When dust accumulates on the Cu precipitate for a period of one week, it adds additional mass when weighed. This is because dust has mass, and as more and more dust accumulate, the accumulation of dust will have a greater mass. As a result, the experimental mass of Cu produced would be greater than the theoretical value of Cu produced in the reaction since the precipitate weighed on the electronic balance is also considering the mass of
A test tube containing 0.2 gram of manganese dioxide was weighed. After recording the data, 1 gram of the unknown substance was then added into the test tube and weighed again, the data recorded also. The test tube was heated using a gas burner and was held by the clamps of the iron stand. The heating continued until there was no more gas rising out of the mouth of the tube which signified that the chemical reaction had already ceased. The test tube was set aside, allowing it to cool to room temperature. When it had reached room temperature, it was weighed and the data recorded. After recording the weight of the test tube and its contents after heating, a second test tube was also weighed with 0.2 gram of manganese dioxide in it. The data was then recorded. A second unknown which is a mixture of potassium chlorate and potassium chloride weighing 2 grams was then placed on the test tube, it was weighed and the data recorded as well. It was held by the clamps on the iron stand and heated using the gas burner. Similar with the first part of the experiment, it was heated until there was no more gas ascending out of the test tube. It was allowed to reach room temperature. The test tube was the weighed and data recorded.
in the experiment of the Atomic Wight of the Element Silver. We react excess amount of copper with silver nitrate solution. To determine the amount of copper reacted and silver that is produced. The first thing that we did was rinsed 150 ml beaker with distilled water. Second, we dispense 10.00 ml of silver nitrate into rinsed beaker. Then we added 100 ml of distilled water to the beaker. Third we obtain a precut copper wire and then winded around large wide mouth test tube to produce a helix or coil of wire. After that we weighed the wire which is 2.1290g in balance number 5. Fourth, we placed the copper wire in the beaker containing dilute silver nitrate solution at 11:30 and then we taped on the copper wire to dislodge the silver metal into
Allow the crucible to cool. Weigh the crucible, its lid, and the product of the reaction.
The purpose of performing this lab was to find the specific heat capacity of an unknown metal.
Theoretical yield is the maximum amount of product that can be produced during a reaction (French et al. 83). The numbers used to find theoretical yield must be those of the limiting reagent (French et al. 83). Because parts of the material used are inevitably lost during experiments, the actual yield will be smaller than the theoretical yield (French et al. 83). To test the efficiency of the reaction, calculate the percent yield as shown below:
Chemical kinetics is a branch of chemistry that involves reaction rates and the steps that follow in. It tells you how fast a reaction can happen and the steps it takes to make complete the reaction (2). An application of chemical kinetics in everyday life is the mechanics of popcorn. The rate it pops depends on how much water is in a kernel. The more water it has the quicker the steam heats up and causes a reaction- the popping of the kernel (3). Catalysts, temperature, and concentration can cause variations in kinetics (4).
First, put on safety goggles to protect the eyes from the chemicals used in this experiment. To begin the lab, label one 100-mL beaker “HCl” using a beaker marker and add 30 mL of 1.0 M Hydrochloric acid solution to this beaker. Next, label the other 100-mL beaker “Na2S2O3” and pour 30 mL of 0.30 M Sodium thiosulfate solution. Finally, label the 250-mL beaker “H2O” and add 25 mL of Distilled or deionized water into this beaker. After all the beakers have been labeled and filled with their set solutions, place a sheet of white paper underneath the six-well reaction plate and using the black sharpie, draw a “X” under each of the wells. Before beginning the lab, place the six-well reaction plate over the sheet and verify that the six “X’s” can be seen through the plate.
borate) and 1.0 g. of sodium hydroxide in 20 mL of warm water. It may
A precipitation reaction can occur when two ionic compounds react and produce an insoluble solid. A precipitate is the result of this reaction. This experiment demonstrates how different compounds, react with each other; specifically relating to the solubility of the compounds involved. The independent variable, will be the changing of the various chemical solutions that were mixed in order to produce different results. Conversely the dependent variable will be the result of the independent variable, these include the precipitates formed, and the changes that can be observed after the experiment has been conducted. The controlled variable will be the measurement of ten droplets per test tube.
of Copper Sulphate. To do this I plan to work out the amount of water
Determination of thermodynamic values allows for analysis of what makes a reaction spontaneous. In this experiment, the equilibrium constant of the crystallization of potassium nitrate as it ionized in water was found and used to determine enthalpy, entropy, and Gibb’s Free Energy of a reaction. The variables were found by by graphing the solubility of potassium nitrate as a function of time and by utilizing relationships based on the van’t Hoff equation. Based on the determined Ksp of 43.4 the average Gibb’s Free Energy over on six trials was -8.4834 kJ/mol with a 510 % error. Relations based on the graph of ln(k) vs. 1/T(K) showed the enthalpy of the reaction to be +34.78 kJ/mol yielding a 2.30% error, and showed the entropy to be +137.4