A mixture of nitrogen and hydrogen was allowed to come to equilibrium at a given temperature.
3H₂ + N₂ 2NH₃
An analysis of the mixture at equilibrium revealed 2.1 mol N₂,3.2 mol H₂,and 1.8 mol NH₃.How many moles of H₂ were present at the beginning of the reaction?

Question

A mixture of nitrogen and hydrogen was allowed to come to equilibrium at a given temperature.
3H₂ + N₂

A mixture of nitrogen and hydrogen was allowed to come to equilibrium at a given temperature. 3H<sub>2</sub> + N<sub>2</sub> 2NH<sub>3</sub> An analysis of the mixture at equilibrium revealed 2.1 mol N<sub>2</sub>,3.2 mol H<sub>2</sub>,and 1.8 mol NH<sub>3</sub>.How many moles of H<sub>2</sub> were present at the beginning of the reaction? A) 3.2 B) 4.8 C) 5.0 D) 5.9 E) 4.4

2NH₃
An analysis of the mixture at equilibrium revealed 2.1 mol N₂,3.2 mol H₂,and 1.8 mol NH₃.How many moles of H₂ were present at the beginning of the reaction?

Quizplus · Accepted Answer

Let x be the number of moles of H₂ at the beginning of the reaction. At equilibrium, we have: 2.1 mol N₂ / 2 = 1.05 mol N₂ 3.2 mol H₂ - x 1.8 mol NH₃ / 2 = 0.9 mol NH₃ Now we can use the equilibrium constant expression: Kc = [NH₃] / ([H₂]^2 * [N₂]) We know that Kc = 4.5. Plugging in the equilibrium concentrations: 4.5 = (0.9) / ((3.2 - x)^2 * (1.05)) Solving for x, we get x = 5.9 mol H₂. Therefore, the answer is (D), 5.9.

A Mixture of Nitrogen and Hydrogen Was Allowed to Come