Choose the statement that is a misconception about a system in chemical equilibrium. (2 points) The rate of the forward reaction is equal to the rate of the backward reaction. The concentrations of the products and reactants dont change. The values of the products and reactants do not have to match each other. The reactions stop once equilibrium is reached.

The correct answer is "The reactions stop once equilibrum is achieved"

Explanation:

A system is said to have attained equilibrium when the rate of forward reaction is the same/equal to the rate of backward reaction.  The reaction below shows a chemical reaction that is at equilibrium

2N₂O₅ (aq) ⇄ 4NO₂ (aq) + O₂ (aq)

An equilibrium reaction is always a reversible reaction. When the system is at equilibrium (when there is a balance), the concentration of the reactants and products do not change despite the fact that reaction does not stop; what happens however is that the rate at which the reactant(s) are formed (backward reaction) will be equal to the rate at which the product(s) are formed (forward reaction).

From the explanation above, it can be deduced that "The reactions stop once equilibrum is achieved" is a misconception about a system in chemical equilibrium.