Question

write the three application of equilibrium constant Kp or Kc​

Answer 1

Answer:

For a certain chemical reaction, the equilibrium constant is defined as the ratio between the amount of reactant and the amount of product which is used to determine chemical behavior.

At equilibrium, Rate of the forward reaction = Rate of the backward reaction

i.e. rf = rb Or, kf × α × [A]a[B]b = kb × α × [C]c [D]d

At a particular temperature, the rate constants are constant. The ratio of the rate constant of forward reaction to the rate constant of backward reaction should be a constant and is called an equilibrium constant (Kequ).

Table of Content

Formula

Units

△G, Qc and Kc

kc vs kp

Characteristics

Applications

Equilibrium Concentration

Factors Affecting Equilibrium Constant

Equilibrium Constant Formula

Kequ = kf/kb = [C]c [D]d/[A]a [B]b = Kc

where Kc, indicates the equilibrium constant measured in moles per litre.

For reactions involving gases: The equilibrium constant formula, in terms of partial pressure will be:

Kequ = kf/kb = [[pC]c [pD]d]/[[pA]a [pB]b] = Kp

Where Kp indicates the equilibrium constant formula in terms of partial pressures.

Larger Kc/Kp values indicate higher product formation and higher percentage conversion.

Lower Kc/Kp values indicate lower product formation and lower percentage conversion.

Medium Kc/Kp values indicate optimum product formation.

Units of Equilibrium Constant

Equilibrium constant being the ratio of the concentrations raise to the stoichiometric coefficients. Therefore, the unit of the equilibrium constant = [Mole L-1]△n.

where, ∆n = sum of stoichiometric coefficients of products – sum of stoichiometric coefficients of reactants.