For the equilibrium reaction: 2NO2(g) ⇌ N2O4(g), what is the effect of increasin

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Question: For the equilibrium reaction: 2NO2(g) ⇌ N2O4(g), what is the effect of increasing the pressure? (2021)

Options:

Correct Answer: Shift to the left

Exam Year: 2021

Solution:

Increasing the pressure will shift the equilibrium to the side with fewer moles of gas, which is the right side (N2O4) in this case.

For the equilibrium reaction: 2NO2(g) ⇌ N2O4(g), what is the effect of increasing the pressure? (2021)

For the equilibrium reaction: 2NO2(g) ⇌ N2O4(g), what is the effect of increasing the pressure? (2021)

Step 1: Identify the reaction: 2NO2(g) ⇌ N2O4(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 NO2.
Step 4: On the right side (products), there is 1 mole of N2O4.
Step 5: Determine which side has fewer moles of gas. The right side has fewer moles (1 mole vs. 2 moles).
Step 6: Understand that increasing pressure in a reaction shifts the equilibrium towards the side with fewer moles of gas.
Step 7: Conclude that increasing the pressure will shift the equilibrium to the right side (N2O4).

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 the relationship between the number of moles of gas on each side of a reaction is crucial for predicting the direction of the shift in equilibrium when pressure changes.