Consider a 70% efficient hydrogen-oxygen fuel cell working under standard conditions at 1 bar and 298 K. Its cell reaction is;

H₂(g) + ½ O₂(g) ? H₂O(l)

The work derived from the cell on the consumption of 1.0 × 10^-3 mol of H₂(g) is used to compress 1.00 mol of a monoatomic ideal gas in a thermally insulated 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.

O₂(g) + 4H+(aq) + 4e^– ? 2 H₂O (l), E^o = 1.23 V

2H+(aq) + 2^– ? H₂(g), E^o = 0.00 V

Use F = 96500 C mol^-1, R = 8.314 J mol^-1 K^-1