Question

2NO3(e) - N:04) +A look in the The text to see what LeChatelict's principle states about gases. Assume that the reaction occurs in an enclosed movable piston. (Hint: remember that PV-RT] a.) The pressure of the reaction is increased. b.) The volume of the reaction is decreased. c.) The volume of the reaction is increased.

Answer 1

Le chatelier principle

Le chatelier principle used to predict the effect of change in condition of chemical equilibrium reactions. Principle states that when system at equilibrium is subjected to changes in terms of concentration, temperature, pressure, volume or pressure equilibrium shifts in direction that tends to counteract the change.

2 NO2---> N2O4+ Heat

a) Pressure of reaction is increased?

From ideal gas law, PV= nRT, states that pressure is proportional to the change in number of moles of reactants and product. When a system is compressed, the total pressure increases, causing the system to shift in the direction that decreases the total number of moles of gas. So product formation is favoured.

b) Volume of reaction is decreased?

Reducing the volume will increase the pressure of reaction which is from ideal gas law equation. Decrease in volume, equilibrium shifts to the side where number of moles is less.

2 NO2--->N2O4+ Heat

From this it is clear number of number of moles of product is greater that number of moles of product. Equilibrium shifts towards right side i.e. product formation is favoured.

c) Volume of reaction is increased?

Increase in volume, equilibrium shifts to the side where number of moles is high.

2 NO2---> N2O4+ Heat

From this it is clear that since number of number of moles of reactants is greater that number of moles of product. This reaction shifts to left.