### Problem 11.43

Posted:

**Wed Nov 30, 2016 1:38 pm**This problem says:

Consider the reaction 2NO2(g)<--->N2(g)+O(g). If the initial pressure of NO is 1.0 bar, and x is the equilibrium concentration of N2, what is the correct equilibrium relation?

The answer is K=x^2/(1.0-2x)^2

My question was: the problem gives the pressure of one and the concentration of the other. Aren't we supposed to convert x to pressure in order to work with the same magnitude?

Consider the reaction 2NO2(g)<--->N2(g)+O(g). If the initial pressure of NO is 1.0 bar, and x is the equilibrium concentration of N2, what is the correct equilibrium relation?

The answer is K=x^2/(1.0-2x)^2

My question was: the problem gives the pressure of one and the concentration of the other. Aren't we supposed to convert x to pressure in order to work with the same magnitude?