Relationship between Kp and Kc:
Consider a common chemical equilibrium reaction, in which the reactants and products are in gaseous phases,aA + bB + cC + ........ ↔ lL + mM + nN + .....then,
Here,p is the partial pressure of the respective gases. In terms of molar concentrations of reactants and products,Kc = ([L]l[M]m[N]n…..)/([A]a[B]b[C]c…..)For some gaseous component ‘i’ in a mixture, its partial pressure ‘pi’ is associated to its molar concentration ‘Ci’ as
Ci = pi/ RT since pi = (ni/V) RT
Here,(ni/V) = Ci = number of moles of i per litre.V = volume in litres.Replacing, concentration in terms by partial pressures,
= Kp/(RT)Δng and,Kp = Kc (RT)Δng
Here,Δng = total number of stoichiometric moles of gaseous products-total number of stoichiometric moles of gaseous reactants.
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