Question

For the reaction N2(g) + 3H2(g) ↔ 2NH3(g), the equilibrium constant, K, = 9.83 x 10-2 at a certain temperature and pressure.

Answer 1

The reaction is not at equilibrium and it is in the forward direction.

a.

Given,

[N₂] = 0.910 mol / L

[H₂] = 0.3 mol / L

[NH₃] = 0.0081 mol / L

K = 9.83 x 10⁻²

The balanced chemical equation for the given reaction is,

N₂(g) + 3H₂(g) ⇄ 2NH₃(g)

The formula of equilibrium constant is given by,

K = [NH₃]² / [N₂] [H₂]²

9.83 x 10⁻² = [(0.0081)² ]/ [0.910 × (0.3)²]

⇒9.83 x 10⁻² = (0.00006561) / (0.0819)

⇒9.83 x 10⁻² = 0.0008010989

⇒0.00983 = 0.0008010989

LHS ≠ RHS

Hence, the reaction is not at equilibrium.

b.

The reaction is in forward direction.

Learn more about direction of the reaction from the link given below.

brainly.com/question/10278602

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