At equilibrium a mixture of n2, h2, nh3 gas at 500◦c is determined to consist of 0.551 mol/l of n2, 0.400 mol/l of h2, and 0.184 mol/l of nh3. what is the equilibrium constant for the reaction

The balanced equation for the reaction is

N₂ (g) + 3H₂ (g) ⇄ 2NH₃ (g)

The equilibrium constant, k for the reaction can be written as

k = [NH₃ (g) ]² / [N₂ (g) ][H₂ (g) ]³

The given concentration are at equilibrium state. Hence, we can use those directly for the calculation.

[NH₃ (g) ] = 0.184 mol/L

[N₂ (g) ] = 0.551 mol/L

[H₂ (g) ] = 0.400 mol/L

By applying the formula,

k = (0.184 mol/L) ² / ((0.551 mol/L) x (0.400 mol/L) ³)

k = 0.960 mol⁻² L²

Hence, the equilibrium constant for the reaction at 500 °C is 0.960 mol⁻² L²