Question

The standard e.m.f of a cell, involving one electron change is found to be $0.591\, V$ at $25^{\circ}C$. The equilibrium constant of the reaction is $(F = 96,500 \,C \,mol^{-1} : R = 8.314\, JK^{-1} \,mol^{-1})$

• A. $1.0×10^1$
• B. $1.0×10^{30}$
• C. $1.0×10^{10}$
• D. $1.0×10^5$

Answer 1

Answer: (C)

$\therefore log \,K_{eq} = \frac{nE^{\circ}}{0.0591} = \frac{1\times0.591}{0.0591}$
$⇒ K_{eq} = 10^{10}$