Question

Consider the reaction below. upper c upper c l subscript 5 (g) double-headed arrow upper p upper c l subscript 3 (g) plus upper c l subscript 2 (g). at 500 k, the reaction is at equilibrium with the following concentrations. [pci5]= 0.0095 m [pci3] = 0.020 [ci2] = 0.020 m what is the equilibrium constant for the given reaction? 0.042 0.42 2.4 24

Answer 1

The equilibrium constant for the given reaction is 0.0421.

What is equilibrium constant?

Equilibrium constant of any reaction is define as the ration of the product of concentration of products to the product of the concentration of reactants, with raise to the respective coefficients.

Given chemical reaction is:
PCl₅ → PCl₃ + Cl₂

The equilibrium constant's for this reaction is:

Kc = [PCl₃] [Cl₂] / [PCl₅], where

Concentration of [PCl₃] = 0.020M

Concentration of [Cl₂] = 0.020M

Concentration of [PCl₅] = 0.0095M

Putting all these values in the above equation we get,

Kc = (0.02 x 0.02) / 0.0095 = 0.0421

Hence, 0.0421 is the equilibrium constant.

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Answer 2

Answer:

A on edg

Explanation:

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