Question

Consider the reaction: S(s) O2(g)SO2(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, Ka and Kb, for reactions a and b below: a.) 2 S(s) 3 O2(g) 2 SO3(g) Ka b.) SO2(g) 1/2 O2(g) SO3(g) Kb

Answer 1

`Ka=([SO_3]^2)/([O_2]^3) \\\\Kb=([SO_3]^3)/([SO_2][O_2]^(1/2))`

Step-by-step explanation:

Hello!

In this case, according to the reactions:

a.) 2 S(s) 3 O2(g) ⇔ 2 SO3(g) Ka

b.) SO2(g) + 1/2 O2(g) ⇔ SO3(g) Kb

Thus, according to the law of mass action, we can write Ka and Kb as follows:

`Ka=([SO_3]^2)/([O_2]^3) \\\\Kb=([SO_3]^3)/([SO_2][O_2]^(1/2))`

Whereas solid carbon is not inserted in the equilibrium expression.

Best regards!