Kp

Kp Used for gaseous equilibria Doesn’t use concentration Instead uses partial pressures p(A) Kp =  p(NH3)2 / p(N2) x p(H2)3 for the reaction N2 +3H2(g) à 2NH3(g) P(A) = Mole fraction (A) x total pressure p 1 mole of gas = 24 dm3 Partial pressure is the contribution each gas makes towards the total pressure. Pa = Pascals kPa = Kilopascals atm = Atmospheres Heterogeneous equilibria Contains species in different states Liquids and solids are omitted