Which of the following changes will shift the equilibrium to the right for the reaction: N2(g) + 3H2(g) ⇌ 2NH3(g)?

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Q: Which of the following changes will shift the equilibrium to the right for the reaction: N2(g) + 3H2(g) ⇌ 2NH3(g)?

Solution: Increasing pressure shifts the equilibrium to the side with fewer moles of gas, which is the right side in this case.

Steps: 7

Step 1: Identify the reaction: N2(g) + 3H2(g) ⇌ 2NH3(g).
Step 2: Count the number of gas molecules on each side of the reaction.
Step 3: On the left side (reactants), there are 1 N2 and 3 H2, totaling 4 gas molecules.
Step 4: On the right side (products), there are 2 NH3, totaling 2 gas molecules.
Step 5: Determine which side has fewer gas molecules. The right side has fewer (2 vs. 4).
Step 6: Understand that increasing pressure in a reaction shifts the equilibrium towards the side with fewer gas molecules.
Step 7: Conclude that increasing pressure will shift the equilibrium to the right side (2NH3).