For the reaction mc011-1.jpg at 472°C equilibrium is established when [H2] =0.0200M, [N2] = 0.0100M and [NH3] = 5.37 x 10-8M. What is the equilibrium constant for this reaction

To find the equilibrium constant (K) for a reaction, we need to know the equilibrium concentrations of the reactants and products. In this case, we are given the equilibrium concentrations of H2, N2, and NH3.

The balanced equation for the reaction is:

N2(g) + 3H2(g) <-> 2NH3(g)

From the given information, we have:

[H2] = 0.0200 M
[N2] = 0.0100 M
[NH3] = 5.37 x 10^-8 M

Using the equilibrium concentrations, we can calculate the equilibrium constant (K) using the formula:

K = ([NH3]^2) / ([N2] * [H2]^3)

Substituting the given concentrations into the formula, we get:

K = ((5.37 x 10^-8)^2) / ((0.0100) * (0.0200^3))

Calculating this expression will give you the equilibrium constant for the reaction.