Question

Which two statements are true for reversible reactions that reach dynamic

equilibrium?
I A. The products of the forward and backward reactions remain
constant at equilibrium.
B. The products of the forward reaction form more quickly than its
reactants.
C. The rate of the forward reaction is greater than the rate of the
backward reaction.
- D. The rate of the forward reaction is equal to the rate of the
backward reaction at equilibrium.

Answer 1

For reversible reactions in dynamic equilibrium, concentrations of reactants and products remain constant, and the rates of forward and reverse reactions are equal.

Step-by-step explanation:

For reversible reactions that reach dynamic equilibrium, two significant truths emerge:

• The concentrations of reactants and products remain constant over time though not necessarily equal, meaning A and B transform into C and D and vice versa at a steady rate.
• The rate of the forward reaction is identical to the rate of the reverse reaction at equilibrium, establishing a state in which the ongoing simultaneous reactions do not result in a net change in concentrations.

Therefore, the two correct statements are (A) The products of the forward and backward reactions remain constant at equilibrium, and (D) The rate of the forward reaction is equal to the rate of the backward reaction at equilibrium. These underline the dynamic nature of a chemical equilibrium where reactions continue, but apparent change is absent since the processes are balanced.