Question

le chatelier's principle question.

3NO->N2O+NO2 (all gas, exothemic reaction)

1)Add inert gas to the equilibrium mixture while maintaining constant overall pressure and temperature.

2)Add inert gas to the equilibrium mixture without changing volume.

1) <- (left) 2) no reaction are the answer, please explain why...!!!!!

+ Please correct my oppinion

Answer 1

Given equation,

3NO----->N₂O + NO₂

1) when an inert gas is added to the equilibrium at constant pressure and temperature, then the total volume of the system will increases. Hence, the number of moles of reactants and products per unit volume will decreases. Here, the number of moles of reactants are more than that of products. Hence the equilibrium shifts towards reactants since more number of moles are present at reactants side. Hence, equilibrium shifts towards left side.

2) When inert gas is added to the equilibrium mixture at constant volume, then the pressure will be increased but the total volume is constant. Hence, the number of moles per unit volume doesn't changes and equilibrium won't changes. Hence, there is no reaction.