Equilibrium Constant Relationship: Kp and Kc

Equilibrium Constant Relationship: Kp and Kc

Equilibrium constants are essential in understanding the balance between reactants and products in a reversible reaction. For the given gaseous reaction COCl2(g) ⇌ CO(g) + Cl2(g), the question asks for the expression of the equilibrium constant Kp in terms of the equilibrium constant Kc.

Expression for Kp in terms of Kc: The relationship between Kp and Kc is determined by the change in the number of moles of gas (Δn) in the reaction. For this specific reaction, the change in the number of moles of gas is equal to 1.

The equation that relates Kp and Kc is represented as: Kp = Kc(RT)^Δn, where R is the ideal gas constant and T is the temperature in Kelvin. In this case, since Δn is equal to 1, the correct expression for Kp in terms of Kc is Kc(RT).

Therefore, the correct answer to the question is Kc(RT), which corresponds to option A among the provided choices.

Understanding the relationship between equilibrium constants such as Kp and Kc is crucial for determining the direction and extent of a chemical reaction at equilibrium. This knowledge allows chemists to make predictions about the behavior of reactants and products in a system under specific conditions.