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Question 5

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)+H2​O(g)⇌CO(g)+3H2​(g)ΔH=+206 kJ mol−1

The 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?

A

Lower rate of reaction and increased yield of hydrogen.

B

Higher rate of reaction and decreased yield of hydrogen.

C

Higher rate of reaction and increased yield of hydrogen.

D

Lower rate of reaction and decreased yield of hydrogen.

Markscheme

Equilibria Questions

  1. GCSE
  2. /Chemistry
  3. /Equilibria

25 exam-style questions on OCR GCSE Chemistry Equilibria. Each one has a worked solution and a mark scheme showing where the marks go.

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