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>-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 value of K is very small, it means the product concentration is much less than the reactant concentration. Therefore, initially the reaction will proceed to the left to try to reach equilibrium.

Consider the Following Equilibrium