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A mixture initially contains A , B , and C in the following concentrations: [A]=0.650mol L−1 , [B]=0.650mol L−1 , and [C]=0.550mol L−1 . The following reaction occurs and equilibrium is established:
A(aq)+2B(aq)⇌C(aq)

At equilibrium, [A]=0.470mol L−1 and [C]=0.730mol L−1 . Calculate the value of the equilibrium constant, Kc .
Express your answer numerically.

Respuesta :

pstnonsonjoku

The equilibrium constant of the solution is obtained as 7.

What is the equilibrium constant?

We know that the equilibrium constant is the constant that shows how much of the reactant has been converted into products in the reaction. We know that we can be able to use the ICE table to obtain the concentration of the substances at equilibrium.

We know that the concentrations at equilibrium would be;

[A]= 0.470mol L−1

[B]= 0.470mol L−1

[C]=0.730mol L−1

Kc = [C]/[A] [B]^2

Kc = 0.730/(0.470)^3

Kc = 7

Learn more about equilibrium constant:https://brainly.com/question/10038290

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