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 * 10^(-4)`.

Step-by-step 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 = ([SO_(2)]^(2)[O_(2)])/([SO_(3)]^(2))`

Substitute the given values into above expression as follows.

`K = ([SO_(2)]^(2)[O_(2)])/([SO_(3)]^(2))\\= (((0.210)/(15.4))^(2) * ((0.354)/(15.4)))/(((8.51 * 10^(-2))/(15.4)))\\= 7.74 * 10^(-4)`

Thus, we can conclude that the value of equilibrium constant, K, is
`7.74 * 10^(-4)`.