For the reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g), what will happen if the volume of t

For the reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g), what will happen if the volume of the container is increased? (2020)

For the reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g), what will happen if the volume of the container is increased? (2020)

Step 1: Understand the reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g). This means that 2 moles of sulfur dioxide (SO2) and 1 mole of oxygen (O2) can produce 2 moles of sulfur trioxide (SO3).
Step 2: Identify the total number of gas moles on each side of the reaction. On the left side (reactants), there are 2 moles of SO2 + 1 mole of O2 = 3 moles of gas. On the right side (products), there are 2 moles of SO3.
Step 3: Recognize that increasing the volume of the container decreases the pressure inside the container.
Step 4: Apply Le Chatelier's principle, which states that if a system at equilibrium is disturbed, it will shift in a direction that counteracts the disturbance.
Step 5: Since increasing the volume decreases the pressure, the equilibrium will shift towards the side with more moles of gas to increase the pressure back.
Step 6: Determine which side has more moles of gas. The left side has 3 moles (2SO2 + 1O2) and the right side has 2 moles (2SO3).
Step 7: Conclude that the equilibrium will shift to the left side (reactants) because it has more moles of gas.

Le Chatelier's Principle – A principle stating that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.
Gas Laws – Understanding how changes in volume affect pressure and the behavior of gases in a reaction.
Stoichiometry of Gases – Analyzing the number of moles of gas on each side of a chemical equation to predict shifts in equilibrium.