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In an excess of hydrogen gas, increasing the amount of chlorine gas in the system will cause the equilibrium to shift to the right. Let's break it down:
1. The reaction given is: H2(g) + Cl2(g) → 2HCl(g)
2. When there is an excess of hydrogen gas, it means there is more hydrogen gas present than needed for the reaction.
3. Increasing the amount of chlorine gas will allow more HCl to be formed according to Le Chatelier's Principle, which states that if a system at equilibrium is subjected to a change, the equilibrium will shift to counteract the change and establish a new equilibrium.
4. Adding more chlorine gas will drive the reaction to the right to consume the excess hydrogen gas, resulting in the formation of more HCl until a new equilibrium is reached with higher HCl concentration.
Therefore, in this scenario, increasing the amount of chlorine gas will cause the equilibrium to shift to the right to counteract the change and establish a new equilibrium with more HCl being produced.
