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

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

Options:

Correct Answer: Shift to the right

Solution:

Increasing the pressure will shift the equilibrium towards the side with fewer moles of gas, which is the right side in this case (2 moles of SO3).

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

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

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: Compare the number of moles of gas on both sides: 3 moles on the left and 2 moles on the right.
Step 6: Understand that increasing pressure in a reaction shifts the equilibrium towards the side with fewer moles of gas.
Step 7: Since the right side has fewer moles (2 moles of SO3), the equilibrium will shift to the right.

Le Chatelier's Principle – This principle states that if an external change is applied to a system at equilibrium, the system will adjust to counteract that change and restore a new equilibrium.
Mole Count in Gaseous Reactions – Understanding how to count the number of moles of gas on each side of a chemical equation is crucial for predicting the direction of the shift in equilibrium.