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An amount of 1.19 g of Y is deposited at cathode when a charge of 0.075 F was passed through the aqueous solution of Y"* using a current of 4.00 A. Given that the molar mass of is 63.5 g mol', (a) calculate the time required (in minutes) for the deposition of Y at cathode. (b) calculate the volume of oxygen gas evolved at anode at STP.

An amount of 1.19 g of Y is deposited at cathode when a charge of 0.075 F was passed through the aqueous solution of Y"* using a current of 4.00 A. Given that the molar mass of is 63.5 g mol', (a) calculate the time required (in minutes) for the deposition of Y at cathode. (b) calculate the volume of oxygen gas evolved at anode at STP.

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 87QAP: Hydrogen gas is produced when water is electrolyzed. 2H2O(g)2H2(g)+O2(g) A balloonist wants to fill...
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An amount of 1.19 g of Y is deposited at cathode when a charge of 0.075 F was passed through the aqueous solution of Ynt using a current of 4.00 A. Given that the molar mass of Y is 63.5 g mol', (a) calculate the time required (in minutes) for the deposition of Y at cathode. (b) calculate the volume of oxygen gas evolved at anode at STP.
Transcribed Image Text:An amount of 1.19 g of Y is deposited at cathode when a charge of 0.075 F was passed through the aqueous solution of Ynt using a current of 4.00 A. Given that the molar mass of Y is 63.5 g mol', (a) calculate the time required (in minutes) for the deposition of Y at cathode. (b) calculate the volume of oxygen gas evolved at anode at STP.
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