A hydrogen gas electrode (H (g), 1.5 bar) is connected via a salt bridge to a…

CHEMISTRY · Multi-part · AP · Chemistry · Thermodynamics and Electrochemistry · Thermodynamics and Electrochemistry

Problem

A hydrogen gas electrode (H

_2

(g), 1.5 bar) is connected via a salt bridge to a chlorine gas electrode in which Cl

_2

(g) is bubbled at 0.50 bar through 0.100 M HCl. The temperature of the entire cell is held at 350 K. Standard reduction potentials (25 °C): Cl

_2

(g) + 2 e

^-

→ 2 Cl

^−

E^{\rm o}=+1.36\,{\rm V}

2 H

^+

+ 2 e

^-

→ H

_2

(g)

E^{\rm o}=0.00\,{\rm V}

Assume ideal gas behavior and that the activity of water is 1. The universal gas constant is

R=8.314\;\text{J mol}^{-1}\text{K}^{-1}

and Faraday’s constant is

F=9.6485\times10^{4}\;\text{C mol}^{-1}

. (a) Write the balanced overall reaction occurring in the cell under the given conditions. (b) Determine the number of moles of electrons transferred per mole of overall reaction as written in part (a). (c) Calculate the cell potential at 350 K using the given pressures and concentration.

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