At constant pressure on addition of inert gasif delta n is 0 no changeif delta n not zero then eqilibrium shifts in direction of more no of molesy is that????? isnt volume decreasing???? then it should shift in direction of less no of moles?????

Dear Student

Adding an inert gas into a gas-phase equilibrium at constant volume does not result in a shift.   This is because the addition of a non-reactive gas does not change the partial pressures of the other gases in the container. While it is true that the total pressure of the system increases, the total pressure does not have any effect on the equilibrium constant; rather, it is a change in partial pressures that will cause a shift in the equilibrium. If, however, the volume is allowed to increase in the process, the partial pressures of all gases would be decreased resulting in a shift towards the side with the greater number of moles of gas

when you add inert gas then total pressure remains same but partial pressure decreases hence the equilibrium will shift towards more number of moles.

you can also see like this.....The partial pressures of the gases will decrease and since volume and pressure are inversely proportional the volume will essentially increase and thus the equilibrium would shift to the side with more gas molecules

for example for the reaction 2CO(g) + O2(g) <---> 2CO2(g)

shift will be towards left

All the best.                                                           

AKASH GOYAL

AskiitiansExpert-IITD

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