For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what happens if the pressure is incr

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Question: For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what happens if the pressure is increased?

Options:

Correct Answer: Equilibrium shifts to the right

Solution:

Increasing the pressure will shift the equilibrium to the right, favoring the formation of SO3, as it has fewer moles of gas.

For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what happens if the pressure is increased?

For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what happens if the pressure is increased?

Step 1: Identify the reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g).
Step 2: Count the number of gas molecules on each side of the reaction.
Step 3: On the left side (reactants), there are 2 moles of SO2 and 1 mole of O2, totaling 3 moles of gas.
Step 4: On the right side (products), there are 2 moles of SO3, totaling 2 moles of gas.
Step 5: Understand that increasing pressure in a reaction favors the side with fewer gas molecules.
Step 6: Since the right side has fewer moles of gas (2 moles of SO3) compared to the left side (3 moles of SO2 and O2), the equilibrium will shift to the right.
Step 7: This shift to the right means more SO3 will be produced.

Le Chatelier's Principle – When the pressure of a gaseous equilibrium is increased, the system will shift in the direction that produces fewer moles of gas.
Stoichiometry of Gases – Understanding the relationship between the number of moles of reactants and products in a gas-phase reaction.