The equation that represents the water-gas shift reaction is :
Show Hint
- \(\mathrm{CO(g) + H_2O(g) \xrightarrow[Catalyst]{673\,K} CO_2(g) + H_2(g)}\)
- \(\mathrm{CH_4(g) + H_2O(g) \xrightarrow[Ni]{1270\,K} CO(g) + 3H_2(g)}\)
- \(\mathrm{C(s) + H_2O(g) \xrightarrow{1270\,K} CO(g) + H_2(g)}\)
- \(\mathrm{2C(s) + O_2(g) + 4N_2(g) \xrightarrow{1273\,K} 2CO(g) + 4N_2(g)}\)
The Correct Option is A
Solution and Explanation
Option (2) is steam reforming of methane, option (3) is the production of water gas itself, and option (4) is the production of producer gas.
Answer: (1) \(\mathrm{CO(g) + H_2O(g) \rightarrow CO_2(g) + H_2(g)}\) (673 K, catalyst)
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