Question

I am having a hard time with this problem. I was wondering where I went wrong. The problem says The equilibrium constant, Kc, for the reaction of H2 and N2 is 1.7×10^2 at 225 ∘C.
3H2(g)+N2(g)←→2NH3(g) If the system at equilibrium contains 0.16M H2 and 0.026M N2, what is the concentration of NH3? I know the equation we use is Kc. And I set it up where Kc is times the reactants. I got .018 and the book says that it is wrong.

Answer 1

I did this earlier but I can't find what I posted. Perhaps I punched the wrong button. I didn't get 0.018 either.
Kc = (NH3)^2/(N2)(H2)^3
0.017 = x^2/(0.026)(0.16)^3
and solve for x.

Answer 2

0.14M