Question

For the cell reaction : $2Cu^{+}_{\left(aq\right)} \to Cu_{\left(s\right)}+Cu^{2+}_{\left(aq\right)}$, the standard cell potential is $0.36\, V$. The equilibrium constant for the reaction is

• A. $1.2\times10^{6}$
• B. $7.4\times10^{12}$
• C. $2.4\times10^{6}$
• D. $5.5\times10^{8}$

Answer 1

Answer: (A)

$log\,K_{c}=\frac{nE^{\circ}_{cell}}{0.0591}$
For the given reaction, $n = 1$
$log\,K_{c}=\frac{1\times0.36}{0.0591}=6.09$
$K_{c}=$ antilog $6.09=1.2\times10^{6}$