Steam reforming converts methane to hydrogen via , (per mole of consumed)

CHEMISTRY · Subjective · AP · Chemistry · Thermochemistry · Thermochemistry

Problem

Steam reforming converts methane to hydrogen via CH4(g)+H2O(g)→CO(g)+3 H2(g)\text{CH}_4(g) + \text{H}_2\text{O}(g) \rightarrow \text{CO}(g) + 3\,\text{H}_2(g), ΔH=+206 kJ mol−1\Delta H = +206\,\text{kJ mol}^{-1} (per mole of CH4\text{CH}_4 consumed). An industrial plant aims to produce 4.50×102 kg4.50\times10^{2}\,\text{kg} of H2\text{H}_2 in a single batch, but the overall yield of the process is only 72 %72\,\%. Calculate the minimum quantity of heat (in kJ) that must be supplied to the reactor to meet this production target.

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