What will happen to the equilibrium position of the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) when the pressure is increased?
Practice Questions
1 question
Q1
What will happen to the equilibrium position of the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) when the pressure is increased?
Shift to the left
Shift to the right
No change
Depends on temperature
Increasing pressure shifts the equilibrium towards the side with fewer moles of gas. Here, the right side has 2 moles (NH3) compared to 4 moles (N2 + 3H2), so the equilibrium shifts to the right.
Questions & Step-by-step Solutions
1 item
Q
Q: What will happen to the equilibrium position of the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) when the pressure is increased?
Solution: Increasing pressure shifts the equilibrium towards the side with fewer moles of gas. Here, the right side has 2 moles (NH3) compared to 4 moles (N2 + 3H2), so the equilibrium shifts to the right.
Steps: 7
Step 1: Identify the reaction: N2(g) + 3H2(g) ⇌ 2NH3(g).
Step 2: Count the number of gas moles on each side of the reaction.
Step 3: On the left side (reactants), there are 1 mole of N2 and 3 moles of H2, totaling 4 moles.
Step 4: On the right side (products), there are 2 moles of NH3.
Step 5: Compare the total moles: 4 moles on the left vs. 2 moles on the right.
Step 6: Understand that increasing pressure favors the side with fewer moles of gas.
Step 7: Since the right side has fewer moles (2 moles), the equilibrium will shift to the right.
