Please explain in at least a sentence for each N2O4 --> 2NO2 Consider the following exothermic reaction: State whether the reaction would proceed in the forward direction, reverse direction, or remain the same by: a) (2 pts) Removing some NO2: ____________________ b) (2 pts) Increasing the temperature: ____________________ c) (2 pts) Decreasing the total pressure: ____________________ d) (2 pts) Decreasing the volume of reaction vessel: ____________________ e) (2 pts) Adding some N2O4: ____________________ Solution According to the Le Chatelier;s principle , when the reaction is at equillibrium , any change in the reaction conditions shifts the equillibrium to the direction where the equillibrium can be re-estabilished. a) When NO2 is removed , the reaction proceeds in the forward direction , so that more of NO2 can be formed and equillibrium can be re-estabilished. b) Since the reaction is endothermic , increasing temperature , will shift reaction in reverse direction so that heat can be utilised c) Decreasing the total pressure proceeds reaction in forward direction , so that the pressure can be increased again. d) Decreasing volume , increases pressure , so the reaction proceeds in reverse direction , so that the equillibrium can be re-estabilished. e) Adding some N2O4 proceeds reaction in forward dorection , so that it can be utilised. .