For the equilibrium reaction: H2(g) + I2(g) ⇌ 2HI(g), what is the effect of addi

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Question: For the equilibrium reaction: H2(g) + I2(g) ⇌ 2HI(g), what is the effect of adding more HI?

Options:

Correct Answer: Shifts to the left

Solution:

Adding more HI increases the concentration of products, which shifts the equilibrium to the left to form more reactants.

For the equilibrium reaction: H2(g) + I2(g) ⇌ 2HI(g), what is the effect of adding more HI?

For the equilibrium reaction: H2(g) + I2(g) ⇌ 2HI(g), what is the effect of adding more HI?

Correct Answer: Equilibrium shifts to the left.

Step 1: Identify the reaction: H2(g) + I2(g) ⇌ 2HI(g).
Step 2: Understand that H2 and I2 are reactants, and HI is the product.
Step 3: Recognize that adding more HI increases the amount of product in the reaction.
Step 4: Apply Le Chatelier's principle, which states that if a change is made to a system at equilibrium, the system will adjust to counteract that change.
Step 5: Since we added more HI (the product), the system will try to reduce the concentration of HI.
Step 6: To reduce HI, the equilibrium will shift to the left, favoring the formation of more reactants (H2 and I2).

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.
Equilibrium Shift – Understanding how the addition of products or reactants affects the direction of the equilibrium shift.