An electrolytic cell is constructed using platinum electrodes in an aqueous NaHCO3 solution. The electrolytic cell is attached to a 9V battery for 2.5 hours, producing 55 mL of H₂(g) at 1.00 atm and 298 K. 2HCO3(aq) + 2e → H₂(g) + 2CO3²-(aq) E° = -0.83 V O2(g) + 4CO2(g) + 2H2O(l) + 4e → 4HCO3- (aq) E° = 2.73 V a. Identify the anode reaction, cathode reaction, and cell reaction. Anode: Cathode: Cell: b. Calculate the current running through the cell. c. Calculate the total volume of gas produced during the electrolysis.

An electrolytic cell is constructed using platinum electrodes in an aqueous NaHCO3 solution. The electrolytic cell is attached to a 9V battery for 2.5 hours, producing 55 mL of H₂(g) at 1.00 atm and 298 K. 2HCO3(aq) + 2e → H₂(g) + 2CO3²-(aq) E° = -0.83 V O2(g) + 4CO2(g) + 2H2O(l) + 4e → 4HCO3- (aq) E° = 2.73 V a. Identify the anode reaction, cathode reaction, and cell reaction. Anode: Cathode: Cell: b. Calculate the current running through the cell. c. Calculate the total volume of gas produced during the electrolysis.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter19: The Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 73QRT

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