Given the equilibrium concentrations in the table, what is the equilibrium constant for the synthesis of ammonia at this temperature?

3H2(g) + N2 2NH3(g)

A. 0.0035
B. 0.014
C. 0.066
D. 0.017

what table?

To find the equilibrium constant for the synthesis of ammonia, we need to use the concentrations of the reactants and products at equilibrium. The equilibrium constant expression for the reaction is:

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

Looking at the table of equilibrium concentrations, we can see that [NH3] = 0.20 M, [H2] = 0.050 M, and [N2] = 0.10 M.

Substituting these values into the equilibrium constant expression:

Kc = (0.20)^2 / (0.050^3 * 0.10)

Calculating this expression:

Kc = 0.04 / (0.000125 * 0.10)
= 0.04 / 0.0000125
= 3200

Therefore, the equilibrium constant for the synthesis of ammonia at this temperature is 3200.

None of the answer choices provided (A, B, C, D) match this value, so there may be a mistake in the given choices.