The Keq of a reaction is 4 x 10-7. At equilibrium:
a. the reactants are favored.
b. the products are favored.
c. the reactants and products are present in equal amounts.
d. the rate of the reverse reaction is much greater than the rate of the
forward reaction.
a. the reactants are favored.
Think this through.
Keq = 4.5E-7 = (products)/(reactants)
At equilibrium you know forward rate = reverse rate so d can't be right.
If c is right then products = reactants so K = 1; that is not so and c can't be right.
That leaves either a or b for the answer. For Keq to be such a SMALL number that makes the (products) small and (reactants) large. So the answer is ..........?
The Keq of a reaction is 4 x 10-7. At equilibrium:
To determine how the reactants and products are favored at equilibrium based on the value of Keq, we need to understand what Keq represents.
Keq, also known as an equilibrium constant, is the ratio of the concentrations of products to the concentrations of reactants at equilibrium.
In this case, the Keq of the reaction is 4 x 10^(-7). Since Keq represents the ratio of products to reactants, a higher value of Keq indicates that the products are favored at equilibrium. Conversely, a lower value of Keq indicates that the reactants are favored at equilibrium.
In this scenario, since the Keq value is very small (4 x 10^(-7)), the reactants are favored at equilibrium. Therefore, the correct answer would be:
a. the reactants are favored.