For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what is the effect of increasing the

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Question: For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what is the effect of increasing the pressure?

Options:

Correct Answer: Shifts equilibrium to the right

Solution:

Increasing the pressure will shift the equilibrium to the right, favoring the production of SO3, as it has fewer moles of gas (3 moles to 2 moles).

For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what is the effect of increasing the pressure?

For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what is the effect of increasing the pressure?

Step 1: Identify the reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g).
Step 2: Count the number of gas moles 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.
Step 4: On the right side (products), there are 2 moles of SO3.
Step 5: Compare the total moles: 3 moles (reactants) vs. 2 moles (products).
Step 6: Understand that increasing pressure favors the side with fewer moles of gas.
Step 7: Conclude that increasing the pressure will shift the equilibrium to the right, producing more SO3.

Le Chatelier's Principle – This principle states that if a system at equilibrium is subjected to a change in pressure, temperature, or concentration, the system will adjust to counteract that change and restore a new equilibrium.
Mole Ratio in Gaseous Reactions – Understanding the relationship between the number of moles of reactants and products in a gas-phase reaction is crucial for predicting the effect of pressure changes.