N2 (g) + 3h2 (g) ⇌ 2nh3 (g) the equilibrium constant kc at 375°c is 1.2. starting with [h2]0 = 0.76 m, [n2]0 = 0.60 m and [nh3]0 = 0.48 m, which concentration (s), if any, will have increased when the mixture comes to equilibrium?

Question

Elliot Hawkins

Chemistry

3 January, 12:36

N2 (g) + 3h2 (g) ⇌ 2nh3 (g) the equilibrium constant kc at 375°c is 1.2. starting with [h2]0 = 0.76 m, [n2]0 = 0.60 m and [nh3]0 = 0.48 m, which concentration (s), if any, will have increased when the mixture comes to equilibrium?

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Lyla Proctor · Answer 1

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

Qc = (NH3^2) / { (N2) (H) ^3) }

Qc = 0.48^2 / { (0.60) (0.760^3) } = 0.875

Qc < Kc therefore the equilibrium will shift to the right. This implies that Nh3 concentration will increase