You're asking about the equilibrium constant (K_eq) for the Haber process, the synthesis of ammonia (NH₃) from nitrogen (N₂) and hydrogen (H₂). Here's how to calculate it:

1. Write the balanced chemical equation:

N₂(g) + 3H₂(g) ⇌ 2NH₃(g)

2. Write the expression for K_eq:

K_eq = [NH₃]² / ([N₂] * [H₂]³)

3. Plug in the equilibrium concentrations:

* [NH₃] = 2 M

* [H₂] = 1 M

* [N₂] = You need to know the equilibrium concentration of N₂ to calculate K_eq. It's not provided in your question.

To solve for K_eq, you need the equilibrium concentration of N₂.

Here's why you need all the equilibrium concentrations:

K_eq is a constant that represents the ratio of products to reactants at equilibrium. To calculate it accurately, you need the concentrations of all the species involved at equilibrium.

Let me know if you have the equilibrium concentration of N₂, and I can calculate K_eq for you!