The concentration of CO will decrease in the reaction vessel if CH₄(g) is added, H₂O(g) is removed, or the pressure is increased. Le Chatelier's principle explains these shifts in equilibrium.
In the given chemical equation:
CO(g) + 3H₂(g) ⇄ 1CH₄(g) + H₂O(g)
To determine the actions that will cause the concentration of CO to decrease in the reaction vessel, we need to consider Le Chatelier's principle. According to this principle, if a system at equilibrium is subjected to a change, it will respond by shifting in a way that counteracts the change.
1. Adding CH₄(g) to the reaction vessel:
When CH₄(g) is added to the reaction vessel, according to Le Chatelier's principle, the equilibrium will shift towards the reactants to counteract the increase in the concentration of CH₄. Therefore, the concentration of CO will decrease.
2. Removing H₂O(g) from the reaction vessel:
If H₂O(g) is removed from the reaction vessel, the equilibrium will shift towards the products to counteract the decrease in H₂O concentration. As a result, the concentration of CO will decrease.
3. Increasing the pressure:
If the pressure is increased, the equilibrium will shift towards the side with fewer gas molecules to reduce the pressure. In this case, the reaction will shift towards the product side, decreasing the concentration of CO.