Consider the reaction 2NO2 (g) ⇌ N2O4 (g) For each of the following mixtures of reactants and products at 25°C, predict the direction in which the reaction will shift to reach equilibrium. a. PNO2 = PN2O4 = 1.0 atm b. PNO2 = 0.21 atm, PN2O4 = 0.50 atm c. PNO2 = 0.29 atm, PN2O4 = 1.6 atm

The effects of varying pressure change is outlined below:

Explanation:

Le Chatelier's principle implies that equilibrium will always shift to counteract any changes in the reaction system. In a gaseous system as this, an increment in pressure shifts an equilibrium to the side of the reaction with the fewer number of moles of gas, or higher atmospheric pressure, and vice versa. If the number of moles of gas is the same on both sides of the reaction, pressure has no effect.

Pressure, P of NO2 = P of N2O4: reaction equilibrium remains the same Pressure, P of NO2 is less than N204: reaction shifts to favour reactant Pressure P of NO2 is less than N2O4: Reaction shifts to favour reactant