Question

Which two statements correctly describe a reversible reaction reaching equilibrium in a closed system?

A) Over time, the rate of the reverse reaction becomes greater than the forward reaction.
B) Initially, the concentration of products is low, so the rate of the reverse reaction is also low.
C) Over time, the rates of the forward and reverse reactions equalize.
D) The total mass in the reactor gradually becomes zero because products are removed from closed systems.

Answer 1

Two accurate descriptions of a reversible reaction reaching equilibrium are: initially, product concentration is low, affecting the rate of the reverse reaction; eventually, the rates of both forward and reverse reactions balance out.

Step-by-step explanation:

Two statements that correctly describe a reversible reaction reaching equilibrium in a closed system are:

B) Initially, the concentration of products is low, so the rate of the reverse reaction is also low.

C) Over time, the rates of the forward and reverse reactions equalize.

A reversible reaction at equilibrium has not only reached a point where the concentrations of reactants and products are stable and unchanging, but also where the rate of the forward reaction (reactants converting to products) is equal to the rate of the reverse reaction (products converting back to reactants). This dynamic process means that even though reactions continue to occur in both directions, there is no net change in concentrations over time. The system must be closed, meaning no reactants or products are added or removed, for equilibrium to be maintained.