Answer
Equilibrium constant$(K)$ for a chemical reaction,present in equilibrium,is expressed by the concentrations of products raised to their stoichiometric coefficients divided by the concentrations of the reactants raised to their stoichiometric coefficients which is written by law of mass action.
$K_{c}$ and$K_{p}$ both are two forms of equilibrium constant,only difference is $K_{c}$ is used with respect to concentration in Molarity and $K_{P}$ is used with respect to partial pressure in atmospheres for gaseous reactions.
They are related as $K_{P}$=$K_{c}(RT)^{\Delta n}$
Here ${\Delta n}$ is change of number of moles of gaseous product from gaseous reactant.
Work Step by Step
Conceptual question. No work needed.
