The hydrogen used in industrial processes can be produced by reacting methane with steam.
CH4(g)+H2O(g)⇌CO(g)+3H2(g) \text{CH}_4(\text{g}) + \text{H}_2\text{O}(\text{g}) \rightleftharpoons \text{CO}(\text{g}) + 3\text{H}_2(\text{g}) CH4(g)+H2O(g)⇌CO(g)+3H2(g)In this reaction, the forward reaction is endothermic.
The conditions used for this industrial reaction are:
Explain, in terms of their effects on the rate of attainment of equilibrium and the equilibrium yield of hydrogen, why this reaction is carried out using a catalyst at 800∘C800^\circ\text{C}800∘C rather than without a catalyst at a lower temperature.
Practise Edexcel GCSE Chemistry Reversible reactions and equilibria with exam-style questions for Foundation and Higher tier. 38 questions, matched to the Edexcel GCSE Chemistry (1CH0) specification and written in Paper 1 and Paper 2 style. Every question includes a full worked solution and mark scheme, so you can see where marks are awarded rather than just whether you got the answer right.
