For the equilibrium 2A(g) ⇌ B(g) + C(g), if the volume of the container is decreased, what will happen?
Practice Questions
1 question
Q1
For the equilibrium 2A(g) ⇌ B(g) + C(g), if the volume of the container is decreased, what will happen?
Shift to the left
Shift to the right
No change
Depends on the temperature
Decreasing the volume increases the pressure, and the equilibrium will shift towards the side with fewer moles of gas, which is the right side in this case.
Questions & Step-by-step Solutions
1 item
Q
Q: For the equilibrium 2A(g) ⇌ B(g) + C(g), if the volume of the container is decreased, what will happen?
Solution: Decreasing the volume increases the pressure, and the equilibrium will shift towards the side with fewer moles of gas, which is the right side in this case.
Steps: 6
Step 1: Understand that the reaction is at equilibrium, meaning both the forward and reverse reactions are happening at the same rate.
Step 2: Identify the reaction: 2A(g) ⇌ B(g) + C(g).
Step 3: Count the number of gas molecules on each side of the equation. The left side (reactants) has 2 moles of gas (2A), and the right side (products) has 2 moles of gas (1B + 1C).
Step 4: Recognize that decreasing the volume of the container increases the pressure inside the container.
Step 5: Apply Le Chatelier's principle, which states that if a system at equilibrium is disturbed, it will shift to counteract the disturbance.
Step 6: Since both sides of the reaction have the same number of moles of gas (2 moles), the equilibrium will not shift to either side based on the change in volume.
