Question #23afe

1 Answer
Jul 2, 2017

Answer:

#K_p = 7.01 xx 10^-6#

Explanation:

We're asked to find the value of the #K_p# for a reaction at a certain temperature with given equilibrium partial pressures.

We do so the same way we would if we were solving for #K_c# (the equilibrium constant for concentration). The equilibrium-constant expression here is

#K_p = ([P_ ("H"_2)]^2[P_ ("O"_2)])/([P_ ("H"_2"O")]^2)#

Plugging in the partial pressure values for each species, we have

#K_p = ((0.00450"atm")^2(0.00250"atm"))/(0.0850"atm")^2 = color(blue)(7.01 xx10^-6#