Raghav Dua

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Hey thank u for making my concepts more clear and sorry for late reply.

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

Law of mass action have 2 parts-equilibrium part & reaction rate part The reaction rate part states that rate of a reaction is directly proportional to the product of active masses of the reactants with each reactant term raised to it's stoichiometric coefficient. The rate law states that rate of a reaction is directly proportional to the product of active masses of the reactants with each reactant term raised to some power which may or may not be equal to stoichiometric coefficient of the reactant. Why the two laws are different when we talk about power to which active masses of reactants are raised ? Which law is correct ?