In the reaction H2(g) + I2(g) ⇌ 2HI(g), what happens if the concentration of HI

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Question: In the reaction H2(g) + I2(g) ⇌ 2HI(g), what happens if the concentration of HI is increased?

Options:

Correct Answer: Shift to the left

Solution:

Increasing the concentration of HI will shift the equilibrium to the left to reduce the concentration of HI, according to Le Chatelier\'s Principle.

In the reaction H2(g) + I2(g) ⇌ 2HI(g), what happens if the concentration of HI is increased?

In the reaction H2(g) + I2(g) ⇌ 2HI(g), what happens if the concentration of HI is increased?

Step 1: Understand the reaction: H2(g) + I2(g) ⇌ 2HI(g) means that hydrogen (H2) and iodine (I2) can combine to form hydrogen iodide (HI).
Step 2: Recognize that the reaction can go in both directions: it can produce HI or break down HI back into H2 and I2.
Step 3: Know that equilibrium means the reaction is balanced, and the amounts of H2, I2, and HI remain constant.
Step 4: Le Chatelier's Principle states that if you change the conditions of a reaction at equilibrium, the system will adjust to counteract that change.
Step 5: If you increase the concentration of HI, the system will try to reduce the amount of HI to restore balance.
Step 6: To reduce HI, the reaction will shift to the left, meaning it will produce more H2 and I2 from HI.

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.