For the equilibrium reaction N2O4 (g) ⇀↽ 2 NO2 (g) taking place inside a sealed container fitted with a piston, predict the effect of raising the piston (to increase the volume of the container) on the composition of the mixture. 1. The equilibrium will shift to favor formation of N2O4 (g). 2. There will be no effect on the composition. 3. More information is needed. 4. The equilibrium will shift to favor formation of NO2 (g).

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Amorcita

Physics

28 August, 19:51

For the equilibrium reaction N2O4 (g) ⇀↽ 2 NO2 (g) taking place inside a sealed container fitted with a piston, predict the effect of raising the piston (to increase the volume of the container) on the composition of the mixture. 1. The equilibrium will shift to favor formation of N2O4 (g). 2. There will be no effect on the composition. 3. More information is needed. 4. The equilibrium will shift to favor formation of NO2 (g).

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Charlie Holland · Answer 1

4. The equilibrium will shift to favor formation of NO2 (g)

Explanation:

According to La Chatalier's Principle which states that when an equilibrium system undergoes changes either in temperature, volume or concentration; there will be in a change in the system in order to reach equilibrium.

From the above equation,

N2O4 (g) ⇀↽ 2 NO2 (g)

From the above reaction, there are 2 moles of gaseous product on the left and 1 mole of gaseous reactant.

Therefore, there are more moles of gases in the left hand side than the right hand side.

Because a decrease in volume favors the direction that produces fewer moles, an increase in volume will therefore shift this system towards the side with more moles of gases that is, more products are formed hence, this system will shift to right and produce more moles of products i. e more NO2 (g) formed.