Which of the following statements about the reaction quotient, Q is false? a. The value of Q can be used to predict equilibrium concentrations. b. It has the same expression as Kc. c. Its value is calculated using nonequilibrium concentrations. d. If Q > Kc, the reaction must move to equilibrium by forming more reactants. e. If Q < Kc, the reaction must move to equilibrium by forming more products.

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as [tex]K_{eq}[/tex]

K is the constant of a certain reaction when it is in equilibrium, while Q is the equilibrium quotient of activities of products and reactants at any stage other than equilibrium of a reaction.

[tex]Q_c<K_c[/tex], reaction will move in forward direction and concentration of products will increase.
[tex]Q_c>K_c[/tex], reaction will move in backward direction and concentration of reactant will increase.
[tex]Q_c=K_c[/tex] reaction is at equilibrium.

pstnonsonjoku pstnonsonjoku · Answer 2 · 2021-12-02T13:46:01+01:00

The statement regarding the reaction quotient Q which is false is the statement; "The value of Q can be used to predict equilibrium concentrations".

The equilibrium constant is a value that gives us a hint as to whether the equilibrium lies in the forward or the reverse direction. A large equilibrium constant indicates that the forward reaction is favored while a small equilibrium constant implies that the reverse reaction is favored. The reaction quotient (Q) is a measure of the concentrations of reactants and products under non - equilibrium conditions.

The statement regarding Q which is false is the statement; "The value of Q can be used to predict equilibrium concentrations".

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