Question

Consider this equilibrium: N2O4(g) + heat <---> NO2(g). Initially, a 1.0 L container is filled with 2.0 mol of NO2. As the system approaches equilibrium, what happens to the rate of reaction of NO2 breaking down?

Answer 1

I think the correct answer would be that the rate of reaction decreases and the concentration of N2O4 increases.This is by virtue of the Le Chatelier's Principle. When the temperature is low than the surroundings, the equilibrium would go from right to left.

Answer 2

According to Le Chateliers principle when a stress is applied to system in dynamic equilibrium the equilibrium shifts to remove that stress. So when additional product, NO₂ is added to the given reaction at equilibrium, the equilibrium will shift to the reactant side or the left side of chemical reaction. In that way excess product will get converted to reactants.