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For the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), what will happen if the pressure is

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Question: For the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), what will happen if the pressure is increased?

Options:

  1. Equilibrium shifts to the left
  2. Equilibrium shifts to the right
  3. No change in equilibrium
  4. Equilibrium constant increases

Correct Answer: Equilibrium shifts to the right

Solution: 

Increasing pressure favors the side with fewer moles of gas. In this case, the right side has 1 mole of CH3OH compared to 3 moles on the left, so the equilibrium shifts to the right.

For the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), what will happen if the pressure is

Practice Questions

Q1
For the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), what will happen if the pressure is increased?
  1. Equilibrium shifts to the left
  2. Equilibrium shifts to the right
  3. No change in equilibrium
  4. Equilibrium constant increases

Questions & Step-by-Step Solutions

For the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), what will happen if the pressure is increased?
  • Step 1: Identify the reaction: CO(g) + 2H2(g) ⇌ CH3OH(g).
  • Step 2: Count the number of gas moles on each side of the reaction.
  • Step 3: On the left side (reactants), there are 3 moles: 1 mole of CO and 2 moles of H2.
  • Step 4: On the right side (products), there is 1 mole of CH3OH.
  • Step 5: Compare the total moles: Left side has 3 moles, right side has 1 mole.
  • Step 6: Understand that increasing pressure in a reaction favors the side with fewer moles of gas.
  • Step 7: Since the right side has fewer moles (1 mole), 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 – Understanding how to count the number of moles of gas on each side of a chemical equation is crucial for predicting the direction of the shift in equilibrium when pressure changes.
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