Which of the following statements are TRUE? Group of answer choices Dynamic equilibrium indicates that the amount of reactants and products are equal. A reaction quotient (Q) larger than the equilibrium constant (K) means that the reaction will favor the production of more products. All of the above are true. The equilibrium constant for the forward reaction is equal to the equilibrium constant for the reverse reaction. Dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction.

Question

Danica Ferrell

Chemistry

21 July, 04:07

Which of the following statements are TRUE? Group of answer choices Dynamic equilibrium indicates that the amount of reactants and products are equal. A reaction quotient (Q) larger than the equilibrium constant (K) means that the reaction will favor the production of more products. All of the above are true. The equilibrium constant for the forward reaction is equal to the equilibrium constant for the reverse reaction. Dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction.

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Anastasia Stokes · Answer 1

Below answers are correct.

1) Dynamic equilibrium indicates that the amount of reactants and products are equal.

2) A reaction quotient (Q) larger than the equilibrium constant (K) means that the reaction will favor the production of more products.

3) Dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction

Explanation: Dynamic equilibrium is also called reversible reaction because it moves both in farward as well as in backward direction. Dynamic equilibrium occurs when reactants convert into products and products convert into reactant at the same time. It only occurs when the reaction occurs in closed container.