Chemistry · Electrochemistry · The First Law & Thermochemistry
Problem
Consider a 70% efficient hydrogen-oxygen fuel cell working under standard conditions at 1 bar and 298 K. Its cell reaction is H₂(g) + 1/2 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 O₂(g) + 4H⁺(aq) + 4e⁻ → 2H₂O(l), E⁰ = 1.23 V, and 2H⁺(aq) + 2e⁻ → H₂(g), E⁰ = 0.00 V. Use F = 96500 C mol⁻¹, R = 8.314 J mol⁻¹ K⁻¹.