MCQ
Consider a $70 \%$ efficient hydrogen-oxygen fuel cell working under standard conditions at 1 bar and $298 K$. Its cell reaction is
$H _2( g )+\frac{1}{2} O _2( g ) \rightarrow H _2 O (\ell)$
The work derived from the cell on the consumption of $1.0 \times 10^{-3} mol$ of $H _2( g )$ is used to compress $1.00 mol$ of a monoatomic ideal gas in a thermally insulted container. What is the change in the temperature (in $K$ ) of the ideal gas ?
The standard reduction potentials for the two half-cells are given below.
$\left. O _2( g )+4 H ^{+} \text {(aq. }\right)+4 e ^{-} \rightarrow 2 H _2 O (\ell), E ^{\circ}=1.23 V,$
$\left.2 H ^{+} \text {(aq. }\right)+2 e ^{-} \rightarrow H _2( g ), E ^{\circ}=0.00 V.$
Use $F =96500 C mol ^{-1}, R =8.314 J mol ^{-1} K ^{-1}$
- ✓$13.32$
- B$13.35$
- C$13.40$
- D$13.45$