In the reaction: 2A(g) ⇌ B(g) + C(g), if the volume of the container is decreased, what will happen?
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?
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 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?
Solution: Decreasing the volume increases the pressure, and the equilibrium will shift towards the side with fewer moles of gas, which is the left side in this case.
Steps: 5
Step 1: Understand the reaction: 2A(g) ⇌ B(g) + C(g). This means that 2 moles of gas A can turn into 1 mole of gas B and 1 mole of gas C.
Step 2: Identify the number of gas moles on each side of the reaction. The left side (reactants) has 2 moles of A, and the right side (products) has 1 mole of B + 1 mole of C, which totals 2 moles.
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 total number of moles (2 moles), the equilibrium will not shift to either side based on the number of moles alone.
