Question

Sulfur dioxide and oxygen react to form sulfur trioxide, like this: (g) (g) (g) Also, a chemist finds that at a certain temperature the equilibrium mixture of sulfur dioxide, oxygen, and sulfur trioxide has the following composition: compound pressure at equilibrium Calculate the value of the equilibrium constant for this reaction. Round your answer to significant digits.

Answer 1

`Kp=9.2x10^(-3)`

Step-by-step explanation:

Hello!

In this case, for the undergoing chemical reaction at equilibrium:

`2SO_2(g)+O_2(g)\rightleftharpoons 2SO_3(g)`

Which means that pressure-based equilibrium constant is computed via the following equilibrium expression:

`Kp=(p_(SO_3)^2)/(p_(SO_2)^2p_(O_2))`

Thus, by plugging in the given pressures at equilibrium, the required Kp turns out:

`Kp=(55.0^2)/(70.2^2*66.7)\\\\Kp=9.2x10^(-3)`

Best regards!