Consider the water-gas shift reaction: , where . Which of the following correctly describes the effe — Chemical Equilibrium Chemistry Question
Question
Consider the water-gas shift reaction: $C(s) + H_2O(g) \rightleftharpoons CO(g) + H_2(g)$, where $\Delta H > 0$. Which of the following correctly describes the effect of increasing the total pressure of the system by halving its volume?
Answer: B
💡 Solution & Explanation
For this reaction, the number of gaseous reactant moles is 1 ($H_2O$) and gaseous product moles is 2 ($CO + H_2$). Thus, $\Delta n_g = +1$. Increasing the pressure by halving the volume causes the system to shift towards the side with fewer gaseous moles to reduce pressure. Therefore, the equilibrium shifts in the reverse (backward) direction.
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