Question

In the reaction, $ H_2(g) + Br_2(g) = 2HBr(g) $, what will happen if there is a change in pressure?

• A. Equilibrium moves left
• B. Equilibrium moves right
• C. There is no change in equilibrium
• D. We cannot say

Hint:

In reactions where the number of gas molecules on both sides is the same, a change in pressure will not affect the equilibrium position.

Answer 1

The Correct Option is B

Step 1: Le Chatelier's Principle
Le Chatelier's principle states that if a system at equilibrium is subjected to a change in conditions such as pressure, temperature, or concentration, the system will shift to counteract the change.

Step 2: Analyzing the Reaction
The reaction is: \[ H_2(g) + Br_2(g) = 2HBr(g) \] Here, we have 2 moles of gas on the left side and 2 moles of gas on the right side.
Therefore, a change in pressure will not shift the equilibrium because there is no change in the total number of moles of gas.
Step 3: Conclusion
Thus, there will be no change in the equilibrium position when pressure is changed.