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In the reaction A(g) + B(g) ⇌ C(g), if the pressure is increased, which directio

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Question: 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?

Options:

  1. Shifts to the right
  2. Shifts to the left
  3. No effect
  4. Increases temperature

Correct Answer: Shifts to the right

Solution: 

Increasing pressure will shift the equilibrium to the right, favoring the side with fewer moles of gas.

In the reaction A(g) + B(g) ⇌ C(g), if the pressure is increased, which directio

Practice Questions

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?
  1. Shifts to the right
  2. Shifts to the left
  3. No effect
  4. Increases temperature

Questions & Step-by-Step Solutions

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?
  • 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.
  • Le Chatelier's Principle – This principle states that if an external change is applied to a system at equilibrium, the system will adjust to counteract that change and restore a new equilibrium.
  • Mole Count in Gaseous Reactions – In reactions involving gases, the number of moles on each side of the equation affects how the system responds to changes in pressure.
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