Question

What is the direction of the reaction if k >> 1?

1) Forward reaction is favored
2) Reverse reaction is favored
3) Both forward and reverse reactions are equally favored
4) Cannot be determined

Answer 1

When K is much greater than 1, the forward reaction is favored and the equilibrium shifts to the product side, indicating the reaction's spontaneity in that direction.

Step-by-step explanation:

When examining a chemical reaction at equilibrium and considering the equilibrium constant, denoted as K, we can determine the direction in which the reaction is favored. If K is significantly greater than 1 (k >> 1), it indicates that the concentration of products is much higher than the concentration of reactants, which means the forward reaction is favored. In this scenario, the equilibrium shifts to the product side. This generally correlates with a negative Gibbs free energy change (delta G), signifying that the reaction is spontaneous in the forward direction.

Le Chatelier's principle helps us understand that when a disturbance is applied to a system at equilibrium, the system will adjust to counteract that change and re-establish equilibrium. For example, adding reactants would cause the forward reaction to increase to consume the added reactants, while removing products would cause the forward reaction to increase to replace the removed products, thus favoring the forward reaction further.