what was the initial volume of your copper sample lab report 5

This could be said due to the overwhelming difference in mass and mole of the final and initial moles and mass. The knob that was controlling the heat was constantly turned up and down due to the violent bubbling. Show one sample calculation. There were many sources of error present throughout this experiment. This surplus of water may have resulted in the greater mass and moles of the final solution. 425 0 obj <> endobj

The initial and final moles of Copper should have also been the same.

This information also differs. Mass Of Recovered Copper , 5. This result defies the law of conservation of mass.

The most probable source of error must have been that there were still some solid zinc that did not react with the copper sulfate. The group may have not waited long enough to let all of the product reach to the bottom of the beaker. Make and record your observations on page 5 . Density of post-1982 penny = 7.19 g/mL . After all of the chemical reactions have finished, the final mass of copper was 6.85 grams. Mass Of Evaporating Dish 4. These masses differ quite tremendously.

The goal of this lab was to see if the mass of copper would be same after going through a series of chemical reactions. The time it took to heat did not reach 5 minutes. Following the heating, there were some of the solution that was on the side of the beaker. Purpose: The purpose of this lab is to accurately determine the densities of pre-1982 and post-1982 pennies. The  results deviated from the weight of copper by 4.841 grams. Cu + HNO 3 - The solution became blue. Privacy The pH tester was suppose indicate a color that matches the number 13. In this lab, each group had the initial mass of the copper close to 2.00 grams. Show one sample calculation trial 1 trial 2 trial 3 mass copper chloride (c) Calculate the mass of chlorine. 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 It is believed that the process was known (metallurgy) as early as 4500 BC. 36% 76% 3.7%.76% Not enough information is given to make this calculation. %%EOF The purpose of this lab is demonstrate the use of the conservation of mass through a series of chemical reactions. If you recover 1.8 grams of copper from a reaction where you started with 5.00 grams of copper(II) chloride and an excess of aluminum, what is your percent yield of copper? The initial and final moles of Copper should have also been the same. 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. There was a significant amount of moles in surplus in comparison to the moles of the final product and the initial product. Nitrogen gas was formed. Percent Yield (show Calculations) % Yield-reca Era Mass Cre- \$83 6. The cooling of the solution is also needed to speed up the process of the formation of a solid product. When decanting the solution, it was hard to extract all of the water from the solution. Another error at this time could be that it was not 2 grams. One source of error would be the inaccurate calibration. This may have affected the results due to the lack of acidity. This is a lab report for my General Chemistry class. The initial moles of copper was 0.0315 grams. Question: Post-Lab Report (a) Report The Collected Data With The Correct Uncertainty. One of the error occurred when testing the pH.

Question: REPORT SHEET EXPERIMENT Chemical Reactions Of Copper 6 And Percent Yield - 1. Whether it be miscalculation or careless mistakes, the results were altered in some way that differs from the law of conservation of mass. Many errors would follow.

Show One Sample Calculation Trial 1 Trial 2 Trial 3 Mass Copper Chloride (c) Calculate The Mass Of Chlorine. Density of pre-1982 penny = 8.87 g/mL . The basis behind this experiment is the law of conservation of mass. After putting the copper through many chemical reactions and phase changes, the final mass of the copper was  6.845 grams of copper. The initial mass of copper used in the experiment was 2.004 grams, and the initial moles of copper was 0.0315. Trial Initial Volume Final Volume (mL) Concentration Mass Copper (&/L) 16. Laboratory Report 1 Title: Accurate Measurement of Mass and Volume Part A: The Formula of Hydrated Copper (II) Sulfate Aim: The objective of this experiment is to find out the accurate mass of a solid and to calculate the moles of an unknown. Composition: 95% copper, 5% zinc. & h�bbd``b`�\$V ��@�eH\$�� After the lab was finished, the final mass of the copper was 6.845 g, and the final … h�b```���@r ?�30EY8@܍��+�x�x�� ��Y �I7.���{޲��P�·)�;:,:88X;\$:;<0t5 Create your own unique website with customizable templates. Freezing Point Depression with Antifreeze Lab. A member of the group would use droplets of water to spray down the solution from the sides of the beaker. Another error would be caused during the decanting process. In our case, my group measured out 2.004 grams of copper. After this process, there was a wait time of 5 minutes. Even this small deviation from the ideal amount could cause a difference in calculations. Initial Mass of Copper                                                                                2.004 grams. your copper solution. Percent Yield = (moles of copper recovered.

The initial mass of the copper was 2.004 grams. 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. View desktop site, Post-Lab Report (a) Report the collected data with the correct uncertainty.

There mere weight of this substance could be enough to alter the final weight of the product. 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. This should have been impossible. Terms The percent yield was calculated at 341.9%. These masses differ quite tremendously. All of the copper in precipitate form has been removed. Most of the group’s measurement deviated from the measurement of 2 grams by less than 0.005 grams. There should have only been little deviation from 2.00 grams. The law of conservation of mass says that matter can neither be created or destroyed. 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. Mass Of Copper And Evaporating Dish - 3. The beaker would take a while in order to start heating up.

After all of the chemical reactions have finished, the final mass of copper was 6.85 grams. This could affect the results dramatically. The problem was that there was not a 13 on the scale. Initial Mass Of Copper -2. Post-Lab Report (a) Report The Collected Data With The Correct Uncertainty. 1) Th product of the reaction between copper and nitric acid in step 2  is placed on ice because it is needed to control the temperature of the reaction.

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trial 1 trial 2 trial 3 mass chlorine (d) Calculate the moles of copper () and chlorine (u) and the ratio (w/x).

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0 During the stage when each groups were to heat  their beaker with their mixture in it, the heating was considerably inconsistent. The beaker was to be kept on the heater for 5 minutes, starting when it begins to boil. This could have drastically increased the final weight of the copper. 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. © 2003-2020 Chegg Inc. All rights reserved.

| 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. Pennies dated 1982-present: Composition: 97.5% zinc, 2.5% copper. %PDF-1.5 %���� The initial mass of the copper was 2.004 grams.

In addition the errors above, another source of error may have came from the final weighing process. 6. endstream endobj 426 0 obj <.

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. Doing this added more water to the solution which could have altered the results. Another would be that inside the evaporating dish, there was a crusty, gelatin-like substance that surrounded the dried up solution. The goal of this lab was to see if the mass of copper would be same after going through a series of chemical reactions. b=�: �-��"�n�.��2����b"B�_�j[�1012�%�D�g��` �^ D 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. While stirring the solution with a glass rod, slowly add 15 mL of Dil (6 M) NaOH to precipitated Cu(OH)2. This particular lab report shows my ability to work with quantitative data, and analyze the calculations and measurements from the lab.… The most probable reason for this result is the abundance in the sources of error throughout the experiment. It is important to add the NaOH slowly, because you are adding a base to an acid. The final weight should have been 2.004 grams of copper. If the product is not cooled, the reaction would be too violent to deal with. 10�����`+-x�%e�7�\o����M�a��%|[��MJi?bqP��s ����00���Y��\$��.W@T1 �8. At the start of the lab, each group was to measure as close to 2 grams of copper as possible. 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. Ol A O: 95% (b) Calculate The Mass Of Copper Chloride In The Volume Of Solution Used. Step II (Conducted at your lab bench) 1. The final moles of copper was .1077 moles.

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