Question

The electrode potential of the following half cell at $298\, K$ $X \left| X ^{2+}(0.001 M ) \| Y ^{2+}(0.01 M )\right| Y$ is _____$\times 10^{-2} V$ (Nearest integer)
 Given: $E _{ x ^{2 *} \mid x }^0=-2.36\, V$ 
$ E _{ Y ^{0-1 Y }}^0=+0.36\, V$ 
$\frac{2303 RT }{ F }=0.06 \,V$

Answer 1

Correct Answer: 275

The correct answer is 275.
$X+Y^{2+}\to Y+X^{2+}$
$E_{\text{Cell}}^0=0.36-(-2.36)=2.72V$
$E_{\text{Cell}}=2.72-\frac{0.06}{2}\log \frac{0.001}{0.01}$
$=2.72+0.03=2.75V$
$=275\times 10^{-2}V$