Question

For the reaction 2 A + B <--> C, the equilibrium concentrations are found to be: [A] = 1.8 X 10^-2 M, [B] = 2.4 X 10^-3 M, and [C] = 5.3 X 10^-4 M. What is the value of Keq?

Answer 1

`K_"eq"~=7xx10^2`

Explanation:

We gots the equilibrium...`2A+BrightleftharpoonsC`...

...and we write the equilibrium expression as...

`K_"eq"=([C])/([A]^2[B])`, where `[A]`, `[B]`, and `[C]` are the concentrations AT EQUILIBRIUM.

But the boundary conditions of the problem gives us PRECISELY those concentrations...

`K_"eq"=([C])/([A]^2[B])=(5.3xx10^-4)/((1.8xx10^-2)^2(2.4xx10^-3))=681.6`..

So which side is favoured at equilibrium, products or reactants?