The steam reforming of methane is an endothermic industrial process used to produce hydrogen gas:
CH4(g)+H2O(g)⇌CO(g)+3H2(g)ΔH=+206 kJ mol−1 \text{CH}_4(\text{g}) + \text{H}_2\text{O}(\text{g}) \rightleftharpoons \text{CO}(\text{g}) + 3\text{H}_2(\text{g}) \quad \Delta H = +206\text{ kJ mol}^{-1} CH4(g)+H2O(g)⇌CO(g)+3H2(g)ΔH=+206 kJ mol−1The reaction is typically carried out at a temperature of around 800∘C800^\circ\text{C}800∘C in the presence of a nickel catalyst.
What happens to the rate of the reaction and the equilibrium yield of hydrogen (H2\text{H}_2H2) if the operating temperature is increased to 950∘C950^\circ\text{C}950∘C?
Lower rate of reaction and increased yield of hydrogen.
Higher rate of reaction and decreased yield of hydrogen.
Higher rate of reaction and increased yield of hydrogen.
Lower rate of reaction and decreased yield of hydrogen.