For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what will happen if the volume of th
Practice Questions
Q1
For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what will happen if the volume of the container is increased? (2020) 2020
Equilibrium shifts to the right
Equilibrium shifts to the left
No change in equilibrium
Reaction stops
Questions & Step-by-Step Solutions
For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what will happen if the volume of the container is increased? (2020) 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: Count the total moles of gas on each side of the reaction. On the left side (reactants), there are 2 moles of SO2 and 1 mole of O2, which totals 3 moles. On the right side (products), there are 2 moles of SO3.
Step 3: Note 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 to counteract the disturbance.
Step 5: Since increasing the volume decreases the pressure, the equilibrium will shift to the side with more moles of gas to increase the pressure again.
Step 6: Identify 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 – This principle states that if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust to counteract that change and restore a new equilibrium.
Gas Laws – Understanding how changes in volume affect pressure and the behavior of gases in a chemical reaction.
Equilibrium Shifts – Recognizing how changes in conditions (like volume) can shift the position of equilibrium towards the side with more or fewer moles of gas.
