In the reaction: 2A(g) ⇌ B(g) + C(g), if the volume of the container is decreased, what will happen to the equilibrium?
Practice Questions
1 question
Q1
In the reaction: 2A(g) ⇌ B(g) + C(g), if the volume of the container is decreased, what will happen to the equilibrium?
Shift to the left
Shift to the right
No change
Depends on temperature
Decreasing the volume increases the pressure, and the equilibrium will shift to the side with fewer moles of gas, which is the left side in this case.
Questions & Step-by-step Solutions
1 item
Q
Q: In the reaction: 2A(g) ⇌ B(g) + C(g), if the volume of the container is decreased, what will happen to the equilibrium?
Solution: Decreasing the volume increases the pressure, and the equilibrium will shift to the side with fewer moles of gas, which is the left side in this case.
Steps: 5
Step 1: Understand that the reaction involves gases: 2A(g) ⇌ B(g) + C(g).
Step 2: Identify the number of gas molecules on each side of the reaction. The left side (2A) has 2 moles of gas, and the right side (B + C) has 2 moles of gas as well.
Step 3: Recognize that decreasing the volume of the container increases the pressure inside the container.
Step 4: Apply Le Chatelier's principle, which states that if a system at equilibrium is disturbed, it will shift to counteract the disturbance.
Step 5: 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 pressure changes.
