What is the effect of increasing the pressure on the equilibrium of the reaction: 2N2(g) + 3H2(g) ⇌ 2NH3(g)?
Practice Questions
1 question
Q1
What is the effect of increasing the pressure on the equilibrium of the reaction: 2N2(g) + 3H2(g) ⇌ 2NH3(g)?
Shifts to the left
Shifts to the right
No effect
Increases the rate of reaction
Increasing the pressure will shift the equilibrium to the right, favoring the formation of NH3, as there are fewer moles of gas on the product side.
Questions & Step-by-step Solutions
1 item
Q
Q: What is the effect of increasing the pressure on the equilibrium of the reaction: 2N2(g) + 3H2(g) ⇌ 2NH3(g)?
Solution: Increasing the pressure will shift the equilibrium to the right, favoring the formation of NH3, as there are fewer moles of gas on the product side.
Steps: 7
Step 1: Identify the reaction: 2N2(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 2 moles of N2 and 3 moles of H2, totaling 5 moles of gas.
Step 4: On the right side (products), there are 2 moles of NH3, totaling 2 moles of gas.
Step 5: Understand that increasing pressure in a reaction favors the side with fewer gas molecules.
Step 6: Since the product side (NH3) has fewer moles of gas (2) compared to the reactant side (5), increasing pressure will shift the equilibrium to the right.
Step 7: This shift to the right means more NH3 will be produced.
