Consider the following equilibrium: N₂(g) + 3H₂(g) 2NH₃(g)
With K = 2.3 *10^-⁶. 1.00 mol each of all reactants and products is placed in a 1.00-L container.
Which way will the reaction initially proceed?

Question

Consider the following equilibrium: N₂(g) + 3H₂(g)

Consider the following equilibrium: N<sub>2</sub>(g) + 3H<sub>2</sub>(g) 2NH<sub>3</sub>(g) With K = 2.3 *10<sup>-</sup><sup>6</sup>. 1.00 mol each of all reactants and products is placed in a 1.00-L container. Which way will the reaction initially proceed? A) To the right. B) We need to know the temperature. C) The system is at equilibrium. D) To the left. E) none of these

2NH₃(g)
With K = 2.3 *10^-⁶. 1.00 mol each of all reactants and products is placed in a 1.00-L container.
Which way will the reaction initially proceed?

Quizplus · Accepted Answer

Since the reaction quotient Qc (which is equal to the denominator of the equilibrium constant expression) will initially be greater than the equilibrium constant K, the reaction will proceed in the direction to consume some of the reactants and produce some of the products. This means the reaction will initially proceed to the left. Therefore, the answer is D.

Consider the Following Equilibrium: N2(g) + 3H2(g) 2NH3(g)

Consider the Following Equilibrium: N₂(g) + 3H₂(g) 2NH₃(g)