For the reaction N₂ (g) + 3H₂ (g) ⇌ 2NH₃ (g) what is the value of Kc at 500 ∘C if the equilibrium concentrations are as follows:

[H₂] = 0.50 M, [N₂] = 0.50 M, and [NH₃] = 2.1 M?

Express the equilibrium constant to two significant figures.

Question

Braggs

Chemistry

7 March, 01:59

For the reaction N₂ (g) + 3H₂ (g) ⇌ 2NH₃ (g) what is the value of Kc at 500 ∘C if the equilibrium concentrations are as follows:

[H₂] = 0.50 M, [N₂] = 0.50 M, and [NH₃] = 2.1 M?

Express the equilibrium constant to two significant figures.

+5

Answers (1)

Know the Answer?

Lorena Johnson · Answer 1

Kc = 70

Explanation:

This is the reaction:

N₂ (g) + 3H₂ (g) ⇌ 2NH₃ (g)

Let's make the expression for K, with concentration at equilibrium and in molarity.

Kc = [NH₃]² / [H₂]³. [N₂]

Kc = (2.1) ² / (0.5) ³. 0.5

Kc = 4.41 / 0.0625 → 70

For the reaction N₂ (g) + 3H₂ (g) ⇌ 2NH₃ (g) what is the value of Kc at 500 ∘C if the equilibrium concentrations are as follows:[H₂] = 0.50 M, [N₂] = 0.50 M, and [NH₃] = 2.1 M?Express the equilibrium constant to two significant figures.

For the reaction N₂ (g) + 3H₂ (g) ⇌ 2NH₃ (g) what is the value of Kc at 500 ∘C if the equilibrium concentrations are as follows:

[H₂] = 0.50 M, [N₂] = 0.50 M, and [NH₃] = 2.1 M?

Express the equilibrium constant to two significant figures.