The water-gas reaction needs very high temperatures. The water-gas shift reac tion, aided by a catalyst, can operate effectively at lower temperatures.
The water-gas reaction requires high temperatures for the reaction to proceed effectively:
Reaction Temperature: \( T_1 \approx 1270 \, \text{K} \)
The water-gas shift reaction is typically carried out at lower temperatures in the presence of a catalyst:
Reaction Temperature: \( T_2 \approx 673 \, \text{K} \)
The temperature for the water-gas reaction (\( T_1 \)) is significantly higher than the temperature for the water-gas shift reaction (\( T_2 \)). Therefore:
\( T_1 > T_2 \)
The equilibrium constant for decomposition of $ H_2O $ (g) $ H_2O(g) \rightleftharpoons H_2(g) + \frac{1}{2} O_2(g) \quad (\Delta G^\circ = 92.34 \, \text{kJ mol}^{-1}) $ is $ 8.0 \times 10^{-3} $ at 2300 K and total pressure at equilibrium is 1 bar. Under this condition, the degree of dissociation ($ \alpha $) of water is _____ $\times 10^{-2}$ (nearest integer value). [Assume $ \alpha $ is negligible with respect to 1]
Match List-I with List-II: List-I