1vinay if conc of reactantis more than conc of products then it does not mean that reaction will proceed forward.
here keq is small thus backward reaction is dominant than forward reaction.
For the reaction, A⟺B,Kc=([B])/([A])
Kc<1 ⇒([B])/([A])<1⇒[B]<[A].If the concentration of reactants is more then the reaction must proceed in forward direction. But my book is writing that the reverse reaction is feasible. Which is true?
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23@ vinay , u r making the mistake here.
Kc = [B]e / [A]e
where [B]e and [A]e are conc of B and A at equilibrium resp, but not at any point of time .
that means at equilibrium conc of B is less than conc of A
39What you've written, vinay, is the reaction quotient, and not the equilibrium constant KC. The reaction quotient Q is defined for an instant of time. The equilibrium constant is defined for concentrations at equilibrium and not any other point of time.
39The equilibrium constant is what qwerty wrote.
KC = [B]e[A]e
Q = [B]t[A]t
where e = time of equilibrium and t = any other instant of time.
So while approaching equilibrium, the concentration of B was obviously greater than A. At equilibrium, the concentration of B is less than A.