According to Le Chatelier's Principle Increasing the conc. of a reactant shifts the reaction in forward direction to re establish the equilibrium.Now if one of the reactant is solid and let the reaction be:
A(s)+B(g)------->C(g)+D(g)
In such a case if we apply the equilibrium constant equation in which conc. of a solid reactant at equilibrium is taken as 1,then according to this increasing to decreasing the conc. of solid will have no effect on equilibrium so there should not be any shift in the reaction
Why rule should be applied in such a case ?
Thanks In advance