Answer to Question #182142 in General Chemistry for Shawn

Question

1. Consider the reversible reaction below which is at equilibrium in a chamber.

3 NO (g) ⇄ N2O (g) + NO2 (g)

Do the following disruptions to equilibrium cause the reaction to move to the right to restore equilibrium or to the left to restore equilibrium?  Explain your answer.

1. Some NO (g) is added to the chamber.

1. Some N2O (g) is removed from the chamber.

1. What happens to the amount of NO2 (g) in the chamber for the disruption in part b?

1. Some NO2 (g) is added to the chamber.

1. The pressure of the chamber is increased.

Answer 1

1.When some NO_(g) is added to the chamber the equilibrium shifts to the right in order to reduce stress.

1.When some N₂O_(g) is removed from the chamber the equilibrium shifts to the left to make more products and also to make up for the lose.

1.What happens to the amount of NO2 (g) in the chamber for the disruption in part b?

There is increase in NO_2(g) in the chamber since the equation shifts to the right to simulate more products.

1.When some NO₂ (g) is added to the chamber.

The equilibrium shifts to the right stimulate an increase in reactants.

1.When the pressure of the chamber is increased.

Pressure increase favours the equation shift to the side with few moles ,in this case to the reactants side