At an equilibrium pressure of 4 atm N2O4 dissociates 15% into NO2. At same temperature what will be equilibrium pressure required for 25% dissociation.

Engineering

Chemistry

Le Chateliers Principle

Question

At an equilibrium pressure of 4 atm N₂O₄ dissociates 15% into NO₂. At same temperature what will be equilibrium pressure required for 25% dissociation.

0.7 atm

1.38 atm

3.9 atm

5.3 atm

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$K_{P} = \frac{4 α^{2} \cdot P}{1 - α^{2}} = const .$
or, $\frac{4 \times {(0 .15)}^{2} \times 4}{1 - {(0 .15)}^{2}} = \frac{4 \times {(0 .25)}^{2} \times P}{1 - {(0 .25)}^{2}}$
P = 1.38 atm

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