Question

Consider the following equilibrium system: 3O2(g)  2O3(g); Keq = 1 Which equation compares the concentration of oxygen and ozone?
A. [O2]3 = [O3]2

B. [O2] = [O3]

C. [O2] = [O3]3/2

D. [O2]2 = [O3]3

Answer 1

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 3O2(g) <--> 2O3(g); 

Keq = 1 = [O3]^2/[O2]^3 

So [O2]^3 = [O3]^2 

Thus A) is correct

Answer 2

Answer: $[O_2]^3=[O_3]^2$

Explanation: Equilibrium constant is the ratio of the concentration of products to the concentration of reactants each term raised to its stochiometric coefficients.

For the given reaction:

$3O_2(g)\rightleftharpoons 2O_3(g)$

$K_{eq}=\frac{[O_3]^2}{[O_2]^3}$

Given :$K_{eq}=1$

Thus $1=\frac{[O_3]^2}{[O_2]^3}$

$[O_2]^3=[O_3]^2$