Which one of the following statements about the equilibrium constant,K_p,is false?

Question

Quizplus · Accepted Answer

The statement that is false is D) Total pressures are used in the equilibrium equation in place of molar concentrations. The equilibrium constant (K) is calculated using the concentrations of the reactants and products at equilibrium, not their total pressures. However, the equilibrium constant (K) for a gaseous reaction can also be expressed in terms of partial pressures, using the relationship Kp = Kc(RT)^(Δn), where Δn is the difference between the sum of the stoichiometric coefficients of the gaseous products and the sum of the stoichiometric coefficients of the gaseous reactants. The units of K are dependent on the units of concentration or partial pressure used.

Which One of the Following Statements About the Equilibrium Constant,Kp,is

Which One of the Following Statements About the Equilibrium Constant,K_p,is