Question

Use the rate constants for the forward and reverse reactions to determine whether reactants or products are favored at equiLiBrium in this case: k subscript e q baseline = k forward over k reverse. When k e q is less than 1, the equiLiBrium lies to the left (reactants are favored). When k e q is greater than 1, the equiLiBrium lies to the right (products are favored). When k e q = 1, neither reactants nor products are favored. k forward = 1.5 × 10⁻⁵. k reverse = 2.2 × 10⁻³. Are reactants favored, products favored, or are they equal?

1) Reactants are favored
2) Products are favored
3) Both are equal

Answer 1

The equilibrium constant (Keq) is calculated from the rate constants of the forward and reverse reactions. In this case, Keq is less than 1, meaning that reactants are favored at equilibrium and the system has more reactants when in equilibrium.

Step-by-step explanation:

To determine whether reactants or products are favored at equilibrium, we look at the equilibrium constant (Keq). It is equal to the rate constant for the forward reaction (kforward) divided by the rate constant for the reverse reaction (kreverse). Given that kforward = 1.5 × 10⁻⁵ and kreverse = 2.2 × 10⁻³, we can calculate Keq as follows:

Keq = rac{kforward}{kreverse} = rac{1.5 × 10⁻⁵}{2.2 × 10⁻³}

This calculation results in Keq being less than 1, indicating that the reactants are favored at equilibrium. Since Keq < 1, there are fewer products produced and more reactants remain when the system has reached equilibrium, as indicated by the equilibrium constant's value favoring the reactants side of the reaction (equilibrium lies to the left).