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You are given 5.0 g of a copper complex (Culen)(H2O),2* yso,2 -2H20 Recall from last week and the practice copper complex work you did, you determined there were 0.400 moles of en in 100 grams of the practice copper complex. You dissolve 0.500 g of your practice copper complex in HCI, water, and ethylenediamine as described in the lab manual, producing 10.00 ml of solution. Using colorimetry, you find that the absorbance of Cu is 0.3635. 1st attempt

You are given 5.0 g of a copper complex (Culen)(H2O),2* yso,2 -2H20 Recall from last week and the practice copper complex work you did, you determined there were 0.400 moles of en in 100 grams of the practice copper complex. You dissolve 0.500 g of your practice copper complex in HCI, water, and ethylenediamine as described in the lab manual, producing 10.00 ml of solution. Using colorimetry, you find that the absorbance of Cu is 0.3635. 1st attempt

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Practice Calculations - Practice Copper Complex You are given 5.0 g of a copper complex [Culen)w(H2O),2* yso,2- 2H20 Recall from last week and the practice copper complex work you did, you determined there were 0.400 moles of en in 100 grams of the practice copper complex. You dissolve 0.500 g of your practice copper complex in HCI, water, and ethylenediamine as described in the lab manual, producing 10.00 mL of solution. Using colorimetry, you find that the absorbance of Cu is 0.3635. 1st attempt hl See Periodic Table From the the moles of Cu in 10.00 mL of the solution, use 63.546 g/mol for the molar mass of Cu** to Calculate the mass of Cu2* in the solution: Cu2 in the solution (use 3 s.f. for the values in the Nickel Day 2 Experiment)
Transcribed Image Text:Practice Calculations - Practice Copper Complex You are given 5.0 g of a copper complex [Culen)w(H2O),2* yso,2- 2H20 Recall from last week and the practice copper complex work you did, you determined there were 0.400 moles of en in 100 grams of the practice copper complex. You dissolve 0.500 g of your practice copper complex in HCI, water, and ethylenediamine as described in the lab manual, producing 10.00 mL of solution. Using colorimetry, you find that the absorbance of Cu is 0.3635. 1st attempt hl See Periodic Table From the the moles of Cu in 10.00 mL of the solution, use 63.546 g/mol for the molar mass of Cu** to Calculate the mass of Cu2* in the solution: Cu2 in the solution (use 3 s.f. for the values in the Nickel Day 2 Experiment)
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