consider the chemical equation in equilibrium.\nch₄(g) + h₂o(g) ⇌ co(g) + 3h₂(g)\nwhat will happen to the…
consider the chemical equation in equilibrium.\nch₄(g) + h₂o(g) ⇌ co(g) + 3h₂(g)\nwhat will happen to the equilibrium of this reaction if the pressure is increased?\nthe equilibrium will shift to the left to favor the reverse reaction.\nthe equilibrium will shift to the right to favor the forward reaction.\nthe equilibrium will not be affected by changing the pressure.\nthe equilibrium will not be reestablished after this kind of stress.
Answer
Brief Explanations:
According to Le - Chatelier's principle, when pressure is increased in a gas - phase reaction, the equilibrium shifts to the side with fewer moles of gas. In the given reaction $CH_4(g)+H_2O(g)\rightleftharpoons CO(g) + 3H_2(g)$, there are 2 moles of gas on the left - hand side (1 mole of $CH_4$ and 1 mole of $H_2O$) and 4 moles of gas on the right - hand side (1 mole of $CO$ and 3 moles of $H_2$). So, increasing pressure will shift the equilibrium to the left to favor the reverse reaction.
Answer:
The equilibrium will shift to the left to favor the reverse reaction.