We can treat the equilibrium constant as the ratio of the forward rate constant, kfwd, with respect to
the reverse rate constant, krev. That is: Keq = kfwd / krev. Which statement is true?
a) kfwd > krev
b) kfwd < krev
The answer is A but how would you explain why that is the answer?
To explain why the answer is A, we need to understand the concept of equilibrium and the rates of the forward and reverse reactions.
Equilibrium is a state in a chemical reaction where the concentrations of reactants and products remain constant over time. It represents the point at which the rates of the forward and reverse reactions are equal. The equilibrium constant, Keq, is a measure of the relative concentrations of the reactants and products at equilibrium.
In the equation Keq = kfwd / krev, kfwd represents the rate constant for the forward reaction, while krev represents the rate constant for the reverse reaction. Since Keq represents the ratio of forward and reverse rate constants, a higher Keq value indicates a higher ratio of kfwd to krev.
Therefore, if the equilibrium constant (Keq) is greater than 1, it means that the forward reaction rate constant (kfwd) is greater than the reverse reaction rate constant (krev). This can be mathematically represented as kfwd > krev. Hence, the correct answer is A: kfwd > krev.