For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what happens to the equilibrium position if the pressure is increased?
Practice Questions
1 question
Q1
For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what happens to the equilibrium position if the pressure is increased?
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. In this case, the right side has 2 moles of NH3 compared to 4 moles of reactants.
Questions & Step-by-step Solutions
1 item
Q
Q: For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what happens to the equilibrium position if the pressure is increased?
Solution: Increasing the pressure shifts the equilibrium towards the side with fewer moles of gas. In this case, the right side has 2 moles of NH3 compared to 4 moles of reactants.
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 and 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.
