Question

Which of the following happens when a reaction reaches dynamic equilibrium in a closed system? (4 points)

Group of answer choices

The concentrations of the reactants and products increase.

The concentrations of the reactants and products decrease.

The rate of the forward reaction equals the rate of the reverse reaction.

The rate of the forward reaction is slower than the rate of the reverse reaction.

Answer 1

The rate of the forward reaction equals the rate of the reverse reaction.

What is dynamic equilibrium?

When it comes to chemical reactions, a dynamic equilibrium is a condition in which a reversible reaction produces products and reactants at an equal rate.

Dynamic equilibrium can only be achieved in a closed system. That is, a system in which there are no external influences in form of energy, material, or pressure.

For example, consider the following reversible reaction:

$A + B < --- > C + D$

If the reaction is in dynamic equilibrium, there will not be a net production of reactants and products. In other words, the rate of production of A and B will be the same as the rate of production of C and D.

This is as opposed to static equilibrium in which the production of both reactants and products stops completely after reaching equilibrium.

More on dynamic equilibrium can be found here: https://brainly.com/question/14280660

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