Hey,

So I am really very confused about this question and my teacher can’t explain it to me either, so I’m really hoping someone can help me make sense of it...

1. The equilibrium constant for the decomposition of ammonia is 100 M^2 at 255°C for the equation

\(\ce{2NH3(g) <=> N2(g) + 3H2(g)}\)

a. Write an expression for the equilibrium constant for the equation:

\(\ce{N2(g) + 3H2(g) <=> 2NH3(g)}\)

Soooo, I did this and I got it correct (I would upload a pic but I suck at uploading pictures on this website... please someone direct me to a detailed explanation of how to do so from an iPhone please 🙏🏼)

But I don’t understand part b.

b. Calculate the equilibrium constant for the equation given in part a.

THIS is where I got stuck! I don’t understand how ~spoiler

~ the answer is 0.01M^-2. I understand where the M^-2 comes from but HOW do they get 0.01M?? My teacher said something about a square root or something but I do not get how or why the answer is that!

Maybe I’m just missing out on something super obvious, idk

someone help please.