For the reaction 4HCl(g) ⇌ 2H2(g) + Cl2(g), what is the effect of adding HCl on

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Question: For the reaction 4HCl(g) ⇌ 2H2(g) + Cl2(g), what is the effect of adding HCl on the equilibrium?

Options:

Correct Answer: Shift to the left

Solution:

Adding more HCl will increase the concentration of reactants, causing the equilibrium to shift to the left to consume the added HCl.

For the reaction 4HCl(g) ⇌ 2H2(g) + Cl2(g), what is the effect of adding HCl on the equilibrium?

For the reaction 4HCl(g) ⇌ 2H2(g) + Cl2(g), what is the effect of adding HCl on the equilibrium?

Step 1: Understand that the reaction involves HCl as a reactant and H2 and Cl2 as products.
Step 2: Recognize that the reaction can reach a state called equilibrium, where the rates of the forward and reverse reactions are equal.
Step 3: Know that adding more HCl increases the amount of reactant in the system.
Step 4: According to Le Chatelier's principle, if you add more reactant, the system will try to counteract this change.
Step 5: The system will shift the equilibrium to the left, meaning it will favor the formation of more reactants (HCl) to consume the added HCl.

Le Chatelier's Principle – This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.