Hydrogen gas reacts with iodine gas at constant temperature in a sealed rigid container. The gases are allowed to reach equilibrium according to the equation above.
- Mayya Alocci
- 3 days ago
- 1 min read
H2(g) + I2(g) ⇌ 2 HI(g)
Hydrogen gas reacts with iodine gas at constant temperature in a sealed rigid container. The gases are allowed to reach equilibrium according to the equation above. Which of the following best describes what will happen to the reaction immediately after additional iodine gas is added to the system?
(A) The rates of both the forward and reverse reactions decrease.
(B) The rates of both the forward and reverse reactions do not change.
(C) The rate of the forward reaction becomes greater than the rate of the reverse reaction.
(D) The rate of the forward reaction becomes less than the rate of the reverse reaction.
Solution: According to Le Chatelier's principle, when equilibrium is disturbed, the system will react in such a way as to restore the equilibrium. Iodine gas is on the left of the equation. When more iodine gas is added, the equilibrium will shift to the right to get rid of the extra iodine gas. Therefore, the rate of the forward reaction will increase and become greater than the rate of the reverse reaction. Choice C is the correct answer.
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