Question

Please Help!! Please, this is due in a couple of minutes, please help

If 8.51×10-2 moles of SO3(g), 0.210 moles of SO2, and 0.354 moles of O2 are at equilibrium in a 15.4 L container at 1.25×103 K, the value of the equilibrium constant, K, is ____

Answer 1

Answer: The value of equilibrium constant, K, is $7.74 \times 10^{-4}$.

Explanation:

The reaction equation is as follows.

$2SO_{3}(g) \rightleftharpoons 2SO_{2}(g) + O_{2}(g)$

Now, the expression for equilibrium constant of this reaction is as follows.

$K = \frac{[SO_{2}]^{2}[O_{2}]}{[SO_{3}]^{2}}$

Substitute the given values into above expression as follows.

$K = \frac{[SO_{2}]^{2}[O_{2}]}{[SO_{3}]^{2}}\\= \frac{(\frac{0.210}{15.4})^{2} \times (\frac{0.354}{15.4})}{(\frac{8.51 \times 10^{-2}}{15.4})}\\= 7.74 \times 10^{-4}$

Thus, we can conclude that the value of equilibrium constant, K, is $7.74 \times 10^{-4}$.