Which of the following is true regarding the concentration of products, for a chemical reaction that is already at equilibrium, assuming no disruptions to the equilibrium? * The concentrations of products will not change because there are no more reactants. The concentrations of products will not change because the limiting reactant is gone. The concentrations of products will not change because the forward and reverse rates are equal. The concentrations of products will change continually because of reversibility.

Question

Beamer

Chemistry

15 November, 21:03

Which of the following is true regarding the concentration of products, for a chemical reaction that is already at equilibrium, assuming no disruptions to the equilibrium? * The concentrations of products will not change because there are no more reactants. The concentrations of products will not change because the limiting reactant is gone. The concentrations of products will not change because the forward and reverse rates are equal. The concentrations of products will change continually because of reversibility.

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Answers (1)

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Brennen Cruz · Answer 1

Answer: The concentrations of products will not change because the forward and reverse rates are equal.

Explanation:

A chemical reaction is defined as the combination of different chemical substances to form new products. A chemical reaction is said to be in equilibrium when the rate of forward reaction (formation of products) equals to the rate of backward reaction (formation of reactants). Also, equilibrium can only be reach when the chemical reaction takes place in a closed system. If not, some of the products may escape leading to no reverse reaction. Some properties of the chemical reaction such as concentration, colour, pressure and density can be measured to know if a chemical reaction system is in equilibrium.