Question

For a reaction $A(s)+2B^{\oplus }\to A^{2+}+2B$
$K_c$ has been found to be $10^{12}$. The $E_{\text{cell }}^{\ominus }$ is

• A. $0.354V$
• B. $0.708V$
• C. $0.0098V$
• D. $1.36V$

Answer 1

Answer: (A)

$E=E^{\ominus }-\frac{0.059}{2}\log K$
At equilibrium, $E=0$
$E^{\ominus }=\frac{0.059}{2}\log K=\frac{0.059}{2}\log 10^{12}$
$=\frac{0.059}{2}\times 12=0.354$