Question

For which of the following systems at equilibrium, at constant temperature, will the doubling of the volume cause a shift to the right?

• A. \( H_2(g) + Cl_2(g) \rightleftharpoons 2HCl(g) \)
• B. \( 2CO(g) + O_2(g) \rightleftharpoons 2CO_2(g) \)
• C. \( N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \)
• D. \( 2CuO(s) \rightleftharpoons 2Cu + O_2(g) \)

Hint:

Le Chatelier’s principle states that if a system at equilibrium is disturbed by changing the volume, temperature, or pressure, the system will adjust to counteract the disturbance.

Answer 1

The Correct Option is C

Step 1: According to Le Chatelier’s principle, increasing the volume of a system at equilibrium will shift the equilibrium to the side with more moles of gas.
Step 2: In the case of \( N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \), the left side has 4 moles of gas, and the right side has 2 moles. Therefore, increasing the volume will shift the equilibrium to the right.

Final Answer: \[ \boxed{N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)} \]