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In the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what happens to the equilibrium when

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Question: In the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what happens to the equilibrium when the volume of the container is decreased? (2023)

Options:

  1. Equilibrium shifts to the left
  2. Equilibrium shifts to the right
  3. No change in equilibrium
  4. Equilibrium shifts to the side with more moles

Correct Answer: Equilibrium shifts to the right

Exam Year: 2023

Solution: 

According to Le Chatelier\'s principle, decreasing the volume increases the pressure, and the equilibrium will shift towards the side with fewer moles of gas. In this case, the right side has 2 moles of SO3 compared to 3 moles on the left, so the equilibrium shifts to the right.

In the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what happens to the equilibrium when

Practice Questions

Q1
In the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what happens to the equilibrium when the volume of the container is decreased? (2023)
  1. Equilibrium shifts to the left
  2. Equilibrium shifts to the right
  3. No change in equilibrium
  4. Equilibrium shifts to the side with more moles

Questions & Step-by-Step Solutions

In the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what happens to the equilibrium when the volume of the container is decreased? (2023)
  • Step 1: Understand the reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g).
  • Step 2: Identify the number of gas moles on each side of the reaction.
  • Step 3: Count the moles on the left side: 2 moles of SO2 + 1 mole of O2 = 3 moles total.
  • Step 4: Count the moles on the right side: 2 moles of SO3 = 2 moles total.
  • Step 5: Recognize that decreasing the volume of the container increases the pressure.
  • Step 6: Apply Le Chatelier's principle: the system will shift to reduce the pressure.
  • Step 7: Determine which side has fewer moles of gas: the right side has 2 moles, while the left has 3 moles.
  • Step 8: Conclude that the equilibrium will shift to the right side (towards SO3) because it has fewer moles of gas.
  • Le Chatelier's Principle – This principle states that if a system at equilibrium is subjected to a change in conditions (such as pressure, volume, or temperature), the system will adjust to counteract that change and restore a new equilibrium.
  • Mole Count in Gaseous Reactions – Understanding the relationship between the number of moles of gas on each side of a chemical equation is crucial for predicting the direction of the shift in equilibrium.
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