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  Attainment of Equilibrium in Chemical Reactions

Attainment of Equilibrium in Chemical Reactions:

A chemical reaction in equilibrium includes the opposing reactions. One of the reactions generates the products and is termed as the forward reaction whereas the other generates the reactants from products and is termed as the reverse reaction. The chemical equilibrium is dynamic in nature. At equilibrium condition, reactant and product molecules are both existed in the reaction mixture in definite quantities.

The equilibrium concentrations of reactants and products do not modify under constant pressure, temperature, and catalysts and so on.

Consider a common equilibrium reaction at constant temperature symbolized by,

658_chemical equillibrium.jpg

According to the law of mass action, rate of forward reaction will be:

Rf = kf [A]a [B]b

and the rate of reverse reaction is:

Rr = kr [C]c [D]d

Here,
kf and kr are rate constants of forward and reverse reactions correspondingly.

At equilibrium Rf = Rr
∴ kf [A]a [B]b = kr [C]c [D]d

2100_chemical equillibrium2.jpg


 Kf/Kr = Kc = equilibrium constant
∴ Kc = ( [C]c [D]d )/ ( [A]a [B]b )

This equation of Kc is also termed as equilibrium law equation. Kc is the equilibrium constant stated in terms of molar concentrations of reactants and products. For reactions including gaseous reactants or products or both, it is more suitable to use partial pressures rather than molar concentrations. Therefore Kc in equilibrium law equation becomes Kp that is the equilibrium constant represented in terms of partial pressure.

 

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