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

The correct answer is 275.
X+Y2+→Y+X2+
E Cell0​=0.36−(−2.36)=2.72V
ECell ​=2.72−20.06​log0.010.001​
=2.72+0.03=2.75V
=275×10−2V