1. what is law of mass action?
2.Explain law of chemical equilibrium and derive it.
1)Law of Mass action : This law was given by Guldberg and Waage in 1864. It states that- The rate of reaction is proportional to the product of the active masses of the reactants , each raised to the power to its stoichiometric coefficient as represented by the balanced reaction.
2)Law of chemical equilibrium : It states that- The product of the molar concentration of the products, each raised to the power equal to its stoichiometric coefficient divided by the product of the molar concentrations of the reactants , each raised to the power equal to its stoichiometric coefficient is constant at constant temperature and is called Equilibrium constant.
DERIVATION:
consider the general reversible reaction:
A + B C + D
At equilibrium , suppose the active masses of A, B, C, and D are represented as [A], [B], [C] and [D].
Applying the law of mass action-
Rate at which A and B react together , that is , Rate of forward reaction [A][B]
= Kf [A][B]
where Kf is proportionality constant is called as velocity constant for forward reaction.
Similarly, rate at which C and D react together ,that is, Rate of the backward reaction
= Kb[C][D]
where Kb represents the velocity constant for the backward reaction
At equilibrium,
Rate of forward reaction= Rate of the backward reaction
Kf[A][B]= Kb[C][D]
K=
Where K is Equilibrium Constant
2)Law of chemical equilibrium : It states that- The product of the molar concentration of the products, each raised to the power equal to its stoichiometric coefficient divided by the product of the molar concentrations of the reactants , each raised to the power equal to its stoichiometric coefficient is constant at constant temperature and is called Equilibrium constant.
DERIVATION:
consider the general reversible reaction:
A + B C + D
At equilibrium , suppose the active masses of A, B, C, and D are represented as [A], [B], [C] and [D].
Applying the law of mass action-
Rate at which A and B react together , that is , Rate of forward reaction [A][B]
= Kf [A][B]
where Kf is proportionality constant is called as velocity constant for forward reaction.
Similarly, rate at which C and D react together ,that is, Rate of the backward reaction
= Kb[C][D]
where Kb represents the velocity constant for the backward reaction
At equilibrium,
Rate of forward reaction= Rate of the backward reaction
Kf[A][B]= Kb[C][D]
K=
Where K is Equilibrium Constant