For the equilibrium reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what will happen if the

For the equilibrium reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what will happen if the volume of the container is increased?

For the equilibrium reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what will happen if the volume of the container is increased?

Step 1: Understand the reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g). This means we have 2 moles of SO2 and 1 mole of O2 on the left (reactants) and 2 moles of SO3 on the right (products).
Step 2: Count the total moles of gas on each side. On the left, we have 2 moles of SO2 + 1 mole of O2 = 3 moles of gas. On the right, we have 2 moles of SO3.
Step 3: Know that increasing the volume of the container decreases the pressure inside the container.
Step 4: According to Le Chatelier's principle, if the pressure decreases, the equilibrium will shift to the side with more moles of gas to counteract the change.
Step 5: Since the left side has 3 moles of gas and the right side has 2 moles, the equilibrium will shift to the left (towards the reactants).

Le Chatelier's Principle – This principle states that if a system at equilibrium is subjected to a change in conditions (such as pressure or volume), the equilibrium will shift in a direction that counteracts that change.
Gas Laws – Understanding how changes in volume affect pressure and the behavior of gases in equilibrium reactions.
Stoichiometry of Gases – Recognizing the number of moles of gas on each side of the equilibrium to determine the direction of the shift.