Question

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.

Answer 1

Answer:

The correct statements are :b, c , d, and e.

Explanation:

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 $K_{eq}$

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.

• $Q_c$, reaction will move in forward direction and concentration of products will increase.
• $Q_c>K_c$, reaction will move in backward direction and concentration of reactant will increase.
• $Q_c=K_c$ reaction is at equilibrium.