The rate law is given by R=k[A]^m[ B]^n where m,n needn't be equal to stoichiometric coefficients....but we use r=k[A]^a[ B]^b where a,b are stoichiometric coefficients when we use ratio rate of forward to rate of backward reaction in getting value of equilibrium constant K for any given reaction at equilibrium.....why is it different in both cases...does it mean all equilibrium reactions are elementary reactions? But that isn't possible as many intermediate steps are equilibrium reactions in the mechanism of complex reactions...(adsbygoogle = window.adsbygoogle || []).push({});

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# Rate law

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