Chemical equilibrium

the equilibrium will shift in the direction containing more number of moles

The answer siddhanth has given is not always true.
If inert gas is added at constant volume it will not have any effect on the equilibrium.
eqn. of ideal gas is PV=nRT
total pressure of system,P=p₁+p₂...
As inert gas is added at constant volume the total pressure of the system increases as no. of molecules have increased.
but partial pressures p(nRT/V) of the gases remains same because V & n are same.
As the partial pressures remains same the equilibrium does not shift anywhere

Let inert gas is added to the system at constant pressure. As the total pressure of the gas is constant the partial pressure of the gases decreases(no. of moles in the system increases)i.e.
p=nP/Σn (Σn increase implies p decreases)
To counteract the decrease in pressure, the equilibrium should shift in the direction containing more no. of mole(more moles means more pressure)
Δn=n_p-n_r
Δn<0 backward shift
Δ0=0 no shift
Δn>0 forward shift