In the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what happens to the equilibrium position if the pressure is increased? (2023)
Practice Questions
1 question
Q1
In the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what happens to the equilibrium position if the pressure is increased? (2023)
Shifts to the left
Shifts to the right
No change
Depends on temperature
Increasing the pressure shifts the equilibrium towards the side with fewer moles of gas, which in this case is the right side (2 moles of NH3).
Questions & Step-by-step Solutions
1 item
Q
Q: In the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what happens to the equilibrium position if the pressure is increased? (2023)
Solution: Increasing the pressure shifts the equilibrium towards the side with fewer moles of gas, which in this case is the right side (2 moles of NH3).
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, there are 1 mole of N2 and 3 moles of H2, totaling 4 moles of gas.
Step 4: On the right side, there are 2 moles of NH3.
Step 5: Compare the total moles of gas: 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 of NH3), the equilibrium will shift to the right.
