What is the effect of increasing the pressure on the equilibrium of the reaction

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Question: What is the effect of increasing the pressure on the equilibrium of the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g)?

Options:

Correct Answer: Shifts to the right

Solution:

Increasing the pressure will shift the equilibrium to the right, favoring the formation of SO3, as there are fewer moles of gas on the right side.

What is the effect of increasing the pressure on the equilibrium of the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g)?

What is the effect of increasing the pressure on the equilibrium of the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g)?

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, there are 2 moles of SO2 and 1 mole of O2, totaling 3 moles of gas.
Step 4: On the right side, 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) compared to the left side (3 moles), increasing pressure will shift the equilibrium to the right.
Step 7: This shift to the right means more SO3 will be produced.

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