Question

A sample of PCl₅ was placed in a container and the following reaction was allowed to come to equilibrium. PCl₅(g) ⇌ PCl₃(g) + Cl₂(g) The equilibrium concentrations were found to be [PCl₅] = 4.55 M and [PCl₃] = [Cl₂] = 0.437 M. Calculate Kc for the reaction

Answer 1

To calculate the equilibrium constant (Kc) for the given reaction, use the equilibrium concentrations of the reactants and products. The given concentrations are [PCl₅] = 4.55 M, [PCl₃] = [Cl₂] = 0.437 M. Plugging in the values, the equilibrium constant (Kc) for the reaction is 0.0417.

Step-by-step explanation:

To calculate the equilibrium constant (Kc) for the given reaction, you need to use the equilibrium concentrations of the reactants and products. The given concentrations are [PCl₅] = 4.55 M, [PCl₃] = [Cl₂] = 0.437 M.

The equilibrium constant expression for the reaction is Kc = [PCl₃] * [Cl₂] / [PCl₅].

Plugging in the values, Kc = 0.437 * 0.437 / 4.55 = 0.0417.

Therefore, the equilibrium constant (Kc) for the reaction is 0.0417.

Answer 2

To calculate the equilibrium constant, Kc, for the given reaction PCl₅ ⇌ PCl₃ + Cl₂, use the concentrations of the reactants and products at equilibrium.

Step-by-step explanation:

In order to calculate the equilibrium constant, Kc, for the given reaction, you need to use the concentrations of the reactants and products at equilibrium.

The equation for the reaction is PCl₅(g) ⇌ PCl₃(g) + Cl₂(g). The equilibrium concentrations given are [PCl₅] = 4.55 M, [PCl₃] = 0.437 M, and [Cl₂] = 0.437 M.

To calculate Kc, you need to use the formula:

Kc = ([PCl₃] * [Cl₂]) / [PCl₅]

Plugging in the given values: Kc = (0.437 * 0.437) / 4.55

= 0.0419 (rounded to four significant figures).