Question

At equilibrium, the concentrations of gaseous N2, O2, and NO in a sealed reaction vessel are [N2] 5 3.3 3 1023 M, [O2] 5 5.8 3 1023 M, and [NO] 5 3.1 3 1023 M. What is the value of Kc for the following reaction at the temperature of the mixture
N2(g)+O2(g) <---> 2 NO(g)

Answer 1

Answer:

$Kc=0.948$

Explanation:

Hello,

In this case, for the given chemical reaction, which is:

$N_2(g)+O_2(g) \rightleftharpoons 2 NO(g)$

The law of mass action is:

$Kc=\frac{[NO]^2}{[N_2][O_2]}$

Thus, for the given concentrations we obtain:

$Kc=\frac{(5 3.1 3 1023 M)^2}{(5 3.3 3 1023 M)(5 5.8 3 1023 M)}\\Kc=0.948$

Best regards.