For the reaction: A(g) + B(g) ⇌ C(g) + D(g), if the volume of the container is decreased, what will be the effect on the equilibrium? (2023)

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Shift to the left
Shift to the right
No effect
Increase the concentration of A

Questions & Step-by-step Solutions

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Q: For the reaction: A(g) + B(g) ⇌ C(g) + D(g), if the volume of the container is decreased, what will be the effect on the equilibrium? (2023)

Solution: Decreasing the volume increases the pressure. According to Le Chatelier's principle, the equilibrium will shift towards the side with fewer moles of gas. If there are more moles of gas on the left side, the equilibrium will shift to the left.

Steps: 6

Step 1: Identify the reaction: A(g) + B(g) ⇌ C(g) + D(g).
Step 2: Understand that A, B, C, and D are gases.
Step 3: Recognize that decreasing the volume of the container increases the pressure inside.
Step 4: Recall Le Chatelier's principle, which states that if a system at equilibrium is disturbed, it will shift to counteract the disturbance.
Step 5: Determine the number of moles of gas on each side of the reaction: left side (A + B) has 2 moles, right side (C + D) has 2 moles.
Step 6: Since both sides have the same number of moles of gas, the equilibrium will not shift in either direction.

For the reaction: A(g) + B(g) ⇌ C(g) + D(g), if the volume of the container is decreased, what will be the effect on the equilibrium? (2023)

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Questions & Step-by-step Solutions

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