In the reaction A(g) + B(g) ⇌ C(g), if the pressure is increased, which direction will the equilibrium shift if there are more moles of gas on the left?
Practice Questions
1 question
Q1
In the reaction A(g) + B(g) ⇌ C(g), if the pressure is increased, which direction will the equilibrium shift if there are more moles of gas on the left?
Shifts to the right
Shifts to the left
No effect
Increases temperature
Increasing pressure will shift the equilibrium to the right, favoring the side with fewer moles of gas.
Questions & Step-by-step Solutions
1 item
Q
Q: In the reaction A(g) + B(g) ⇌ C(g), if the pressure is increased, which direction will the equilibrium shift if there are more moles of gas on the left?
Solution: Increasing pressure will shift the equilibrium to the right, favoring the side with fewer moles of gas.
Steps: 7
Step 1: Identify the reaction: A(g) + B(g) ⇌ C(g).
Step 2: Count the moles of gas on each side of the reaction.
Step 3: On the left side (reactants), there are 2 moles of gas (A and B).
Step 4: On the right side (products), there is 1 mole of gas (C).
Step 5: Note that there are more moles of gas on the left side (2 moles) than on the right side (1 mole).
Step 6: Understand that increasing pressure in a gas reaction shifts the equilibrium towards the side with fewer moles of gas.
Step 7: Since the right side has fewer moles of gas, the equilibrium will shift to the right.
