If the ratio of concentration of products to reactants is greater than Kc, what does it mean?
Correct answer: A. More reactants are needed to attain equilibrium
- A. More reactants are needed to attain equilibrium
- B. The reaction is moving backward
- C. There are more reactants in the system
- D. More products are needed to attain equilibrium
Explanation
The equilibrium constant Kc is the ratio of the product of the concentration of products to that of reactants in an equilibrium mixture. The reaction quotient Q is the ratio of the concentration of products to that of reactants at any instant. In a reaction mixture at a particular instant, if: Q > Kc, the [products] > [reactants] the reaction must shift in the reverse direction and increase the concentration of reactants to attain equilibrium. Q = Kc, the reaction is at equilibrium. Q < Kc, the [products] < [reactants] the reaction must shift in the forward direction and increase the concentration of products to attain equilibrium.
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About Chemical Equilibrium
Reversible reactions reach dynamic equilibrium when forward and reverse rates become equal, and Le Chatelier's principle predicts the effect of changing concentration, pressure or temperature. The chapter also covers solubility product, the common ion effect, buffer action and the conditions used in Haber's process, with equilibrium shifts distinguished from changes in the equilibrium constant.
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