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An aqueous solution of copper (II) nitrate was electrolyzed using a current of 1.5 A for 60 minutes at 25°C and 1 atm. Calculate: a) The mass of copper metal deposited at the cathode. b) The volume of gas evolved the anode. (Atomic mass: Cu = 63.5 g/mol) %3D

An aqueous solution of copper (II) nitrate was electrolyzed using a current of 1.5 A for 60 minutes at 25°C and 1 atm. Calculate: a) The mass of copper metal deposited at the cathode. b) The volume of gas evolved the anode. (Atomic mass: Cu = 63.5 g/mol) %3D

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
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Exercise An aqueous solution of copper (II) nitrate was electrolyzed using a current of 1.5 A for 60 minutes at 25°C and 1 atm. Calculate: a) The mass of copper metal deposited at the cathode. b) The volume of gas evolved the anode. (Atomic mass: Cu = 63.5 g/mol)
Transcribed Image Text:Exercise An aqueous solution of copper (II) nitrate was electrolyzed using a current of 1.5 A for 60 minutes at 25°C and 1 atm. Calculate: a) The mass of copper metal deposited at the cathode. b) The volume of gas evolved the anode. (Atomic mass: Cu = 63.5 g/mol)
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