The final weight should have been 2.004 grams of copper. b=�: �-��"�n�.��2����b"B�_�j[�1012�%�D�g��` �^ D Another error at this time could be that it was not 2 grams. %PDF-1.5 %���� Show One Sample Calculation Trial 1 Trial 2 Trial 3 Mass Copper Chloride (c) Calculate The Mass Of Chlorine. The most probable source of error must have been that there were still some solid zinc that did not react with the copper sulfate. Lab #6 Chemical Transformations of Copper Introduction: Copper was one of the first metals to be isolated, due to the ease of separating it from its ores. This may have affected the results due to the lack of acidity. When decanting the solution, it was hard to extract all of the water from the solution. All of the copper in precipitate form has been removed. Show one sample calculation trial 1 trial 2 rial 3 moles of copper moles of chloride mol( chlorine) mol (copper) (e) Report the formula CuCly/, using the average ratio CHM 117 Spring 2018. One of the error occurred when testing the pH. Terms Privacy While stirring the solution with a glass rod, slowly add 15 mL of Dil (6 M) NaOH to precipitated Cu(OH)2. This could be said due to the overwhelming difference in mass and mole of the final and initial moles and mass. After the lab was finished, the final mass of the copper was 6.845 g, and the final … The assignment was to create a formal lab report that expresses data and observations, lab procedure, and a discussion of the data with a conclusion. 10�����`+-x�%e�7�\o����M�a��%|[��MJi?bqP��s ����00���Y��$��.W@T1 �8. These masses differ quite tremendously. 36% 76% 3.7%.76% Not enough information is given to make this calculation. This should have been impossible. The purpose of this lab is demonstrate the use of the conservation of mass through a series of chemical reactions. The percent yield was calculated at 341.9%. If the product is not cooled, the reaction would be too violent to deal with. Many errors would follow. Trial Initial Volume Final Volume (mL) Concentration Mass Copper (&/L) 16. At the start of the lab, each group was to measure as close to 2 grams of copper as possible. The basis behind this experiment is the law of conservation of mass. Make and record your observations on page 5 . Pennies dated 1982-present: Composition: 97.5% zinc, 2.5% copper. The initial mass of copper used in the experiment was 2.004 grams, and the initial moles of copper was 0.0315. In this lab, each group had the initial mass of the copper close to 2.00 grams. 462 0 obj <>stream The beaker would take a while in order to start heating up. Ol A O: 95% (b) Calculate The Mass Of Copper Chloride In The Volume Of Solution Used. Even this small deviation from the ideal amount could cause a difference in calculations. The initial moles of copper was 0.0315 grams. The problem was that there was not a 13 on the scale. There mere weight of this substance could be enough to alter the final weight of the product. After this process, there was a wait time of 5 minutes. Create your own unique website with customizable templates. After all of the chemical reactions have finished, the final mass of copper was 6.85 grams. Initial Mass Of Copper -2. Density of post-1982 penny = 7.19 g/mL . Purpose: The purpose of this lab is to accurately determine the densities of pre-1982 and post-1982 pennies. Due to the Law of Conservation of Mass, one would predict that after any number of chemical reactions and phase changes, the final mass and number of moles of copper would remain the same as the initial amounts. After all of the chemical reactions have finished, the final mass of copper was 6.85 grams. trial initial volume final volume (mL) concentration mass copper () (&/L) 16. ol a O: 95% (b) Calculate the mass of copper chloride in the volume of solution used. Most of the group’s measurement deviated from the measurement of 2 grams by less than 0.005 grams. In addition the errors above, another source of error may have came from the final weighing process. This result defies the law of conservation of mass. Percent Yield (show Calculations) % Yield-reca Era Mass Cre- $83 6. Another would be that inside the evaporating dish, there was a crusty, gelatin-like substance that surrounded the dried up solution. The time it took to heat did not reach 5 minutes. The results deviated from the weight of copper by 4.841 grams. There should have only been little deviation from 2.00 grams. It is important to add the NaOH slowly, because you are adding a base to an acid. A source of error that could be present at this time could have been that the scale was not properly calibrated, thus throwing off the weighted measurement. Percent Yield = (moles of copper recovered. 445 0 obj <>/Filter/FlateDecode/ID[<4964B7B108E29346BB75D38CE0516694>]/Index[425 38]/Info 424 0 R/Length 94/Prev 54442/Root 426 0 R/Size 463/Type/XRef/W[1 2 1]>>stream trial 1 trial 2 trial 3 mass chlorine (d) Calculate the moles of copper () and chlorine (u) and the ratio (w/x). %%EOF The goal of this lab was to see if the mass of copper would be same after going through a series of chemical reactions. & One source of error would be the inaccurate calibration. The law of conservation of mass says that matter can neither be created or destroyed. These masses differ quite tremendously. Nitrogen gas was formed. This particular lab report shows my ability to work with quantitative data, and analyze the calculations and measurements from the lab.… It is a ductile, malleable metal and is easily pounded and/or drawn into various shapes for use as wire, ornaments and implements of various types. Mass Of Evaporating Dish 4. Show one sample calculation trial 1 trial 2 trial 3 mass copper chloride (c) Calculate the mass of chlorine. The initial mass of the copper was 2.004 grams. The result of this copper lab should have been that the mass of the initial copper and the mass of the final copper equals each other. Another error would be caused during the decanting process. Question: REPORT SHEET EXPERIMENT Chemical Reactions Of Copper 6 And Percent Yield - 1. The beaker was to be kept on the heater for 5 minutes, starting when it begins to boil. During the stage when each groups were to heat their beaker with their mixture in it, the heating was considerably inconsistent. The goal of this lab was to see if the mass of copper would be same after going through a series of chemical reactions. This is a lab report for my General Chemistry class. This experiment would involve the use of copper (Cu) in a series of reactions that when finished, should equal the same amount of mass as when first started. This could have drastically increased the final weight of the copper. The initial and final moles of Copper should have also been the same. your copper solution. endstream endobj 426 0 obj <. Doing this added more water to the solution which could have altered the results. The initial and final moles of Copper should have also been the same. h�bbd``b`�$V ��@�eH$�� Cu + HNO 3 - The solution became blue. The most probable reason for this result is the abundance in the sources of error throughout the experiment. Mass Of Recovered Copper , 5. After putting the copper through many chemical reactions and phase changes, the final mass of the copper was 6.845 grams of copper. View desktop site, Post-Lab Report (a) Report the collected data with the correct uncertainty. Density of pre-1982 penny = 8.87 g/mL . The initial mass of the copper was 2.004 grams. Following the heating, there were some of the solution that was on the side of the beaker. The final moles of copper was .1077 moles. © 2003-2020 Chegg Inc. All rights reserved. This could affect the results dramatically. The cooling of the solution is also needed to speed up the process of the formation of a solid product. Whether it be miscalculation or careless mistakes, the results were altered in some way that differs from the law of conservation of mass.
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