Explain about Kp (i.e equilibrium constant in terms of partial pressure)?

Question

It's urgent.

Answer 1

Kp is the ratio of the partial pressures of the products to the partial pressure of the reactants each raised to the power of their coefficients. Kp is used mainly for reactions involving gases e.g consider the gaseous reaction
N2 + 3H2 --------> 2NH3
Kp for this reaction will be:
(P.P of NH3)^2/ ((P.P of N2) x(P.P of H2)^3
where P.P means partial pressure

Answer 2

Kp, like any other equilibrium constant, relates the concentation of products to reactants when a reaction occurs in the gas phase. Since partial pressure relates to concentrations by the ideal gas Law (partial pressure of product or reactant at equilbrium)Vtotal= (moles of product or reactant)RT, measuring these partial pressures can be used to determine Kp in gas just as a K would be determined in liquid.

Answer 3

Kp is set up in a similar manner to the equilibrium constant for concentration. It is a unitless quantity.

Kp = (partial pressures of products)/(partial pressures of reactants)