Which of the following relation is correct forKf and Kb in an equilibrium process that contain equal moles of reactants and products a) Kf=Kb b) KfKb C) kf=Kb d) we cannot predict?

Question

Which of the following relation is correct forKf and Kb in an equilibrium process that contain equal moles of reactants and products a) Kf=Kb b) Kf>Kb C) kf=Kb d) we cannot predict?

Answer

Answer:

Introduction:
In an equilibrium process, the equilibrium constant (K) is defined as the ratio of the concentration of products to the concentration of reactants at equilibrium. The equilibrium constant can be expressed in terms of two equilibrium constants, Kf and Kb, which are the rate constants for the forward and reverse reactions, respectively.

Explanation:
The equilibrium constant for a reaction can be expressed as:

K = [Products]/[Reactants]

Kf and Kb are related to K as follows:

K = Kf/Kb

If the forward and reverse reactions are reversible and occur at the same rate, then Kf = Kb, and K = 1. In this case, the reaction is said to be at equilibrium.

If the forward reaction is faster than the reverse reaction, then Kf > Kb, and K > 1. In this case, the reaction will proceed forward until equilibrium is reached.

If the reverse reaction is faster than the forward reaction, then Kf < kb,='' and='' k='' />< 1.='' in='' this='' case,='' the='' reaction='' will='' proceed='' in='' reverse='' until='' equilibrium='' is='' />

Conclusion:
In an equilibrium process that contains equal moles of reactants and products, the reaction is at equilibrium, and K = 1. Therefore, Kf = Kb. The correct relation is option (a) Kf = Kb.

Answer

For equilibrium kf=kb

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