Give the direction of the reaction, if K ≈ 1. Potential Answers: If the temperature is raised, then the forward reaction is favored. The reverse reaction is favored. The forward reaction is favored. If the temperature is raised, then the reverse reaction is favored. Neither direction is favored.
The Correct Answer and Explanation is:
Correct Answer: Neither direction is favored.
Explanation:
The equilibrium constant, K, provides a measure of the ratio of product concentrations to reactant concentrations at equilibrium. When K ≈ 1, it means that the concentrations of reactants and products are approximately equal at equilibrium. This tells us that the system is balanced and neither the forward nor reverse reaction is strongly favored.
In a chemical equilibrium:
- If K >> 1, products are favored, and the forward reaction predominates.
- If K << 1, reactants are favored, and the reverse reaction predominates.
- If K ≈ 1, neither reactants nor products are strongly favored, and the reaction lies near the center of the equilibrium spectrum.
This balanced position implies that the reaction mixture contains significant amounts of both reactants and products. At this point, the forward and reverse reactions occur at roughly the same rate, so the system is considered dynamic but stable.
The options mentioning temperature changes (e.g., “if the temperature is raised”) involve Le Châtelier’s Principle, which tells us how equilibrium shifts in response to external changes like temperature, pressure, or concentration. However, unless the reaction is explicitly stated to be exothermic or endothermic, we cannot determine the effect of temperature. Since the question only gives the value of K ≈ 1, there is no basis to predict how the system will respond to temperature changes without more data.
Therefore, based solely on the equilibrium constant being close to one, we conclude:
Neither direction is favored, because the system is at a balanced equilibrium with nearly equal concentrations of reactants and products.
