Which of the following statements is true?
a. a reaction quotient (q) larger than the equilibrium constant (k) means that the reaction will favor the production of more products.
b. the equilibrium constant for the forward reaction is equal to the equilibrium constant for the reverse reaction.
c. dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction.
d. dynamic equilibrium indicates that the amount of reactants and products are equal.

Dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction:

Explanation:

Reaction quotient is the ratio of product of concentrations of products to product of concentrations of reactants at any time.

The same ratio at equilibrium (when rate of forward reaction becomes equal to rate of backward reaction) is equilibrium constant.

when Q < Kc, a forward reaction is favored.

When when Q > Kc, a backward or reverse reaction is favored

So the first statement that

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

b) No the rate of forward and backward reaction are equal.

c) c. Dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction: True

d) Dynamic equilibrium indicates that the amount of reactants and products are equal: This could be static equilibrium but not dynamic.

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explanation: