data analysis - Experiment 2: Determination of the...

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Experiment 2: Determination of the Empirical Formula of Copper Chloride Pat Popovits CHM 151LB CRN: 22548 03/05/08 I. Overview In this experiment copper chloride reacted with HCL and Zn to make a solid that is copper. The copper was left in a beaker and the zinc would lose its shine. This was done for 10 minutes in each experiment. In each experiment zinc was weighed and there was approximately 1g of unknown copper chloride used. 25 ml of HCL was also added to complete the reaction. II. Observations III. Data Analysis Questions 1. From the weight of the copper that you obtained in the experiment, determine the number of moles of copper that were present in the copper chloride sample. Report your answer as the average of your three trials. This value will be the variable “x” in the empirical formula of the copper chloride. (0.598+1.005+0.745) / 3 = .7826 (1/63.546) = .0123mol Cu 2. For each trial use the initial weight of the copper chloride sample to determine the weight of chloride in the sample. 1: (1.016-.598) = .418 2: (1-1.005) = -.005 3: (1-.745) = .255 Average: (.418-.005+.255)/3 = .223 Feb 15, 2008 Page 1 of 6 (weight in grams) Experiment 1 Experiment 2 Experiment 3 Cu x Cl y weight used 1.016 1.000 1.000 Zinc (initial weight) 0.737 ? 0.848 Zinc (final weight) 0.324 0.479 0.599 Cu precipitate 0.598 1.005 0.745
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Experiment 2: Determination of the Empirical Formula of Copper Chloride 3. For each trial use the initial weight of the copper chloride sample to determine the weight of chloride in the sample. 1:
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This note was uploaded on 04/02/2008 for the course PHYS 121 taught by Professor Wormer during the Spring '08 term at University of Arizona- Tucson.

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data analysis - Experiment 2: Determination of the...

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