Question

13. Which of the following statements about the equilibrium constant is correct? a. If Keq l there is no reaction. b. If Keq>1 the reaction favors reactant formation c. If Keq>1 the reaction favors product formation. d. both A and C Short Answer/Problems: Consider the exothermic reaction 2 H2 (g) + O2 (g) 2 H2O (g) If the reactio at equilibrium indicate in which direction the reaction would shift, if any, with the following disturbances? B) H2 is removed D) The reaction is heated A) H20 is added C) O2 is added

Answer 1

13.

$K_{eq}=\frac{[Products]}{[Reactants]}$

• If Keq = 1, then the position of equilibrium is in the center, the amount of products is roughly equal to the amount of reactants at equilibrium.
• If Keq is much greater than 1 (For example if Keq = 10³), then the position of equilibrium is to the right; more products are present at equilibrium.
• If Keq is much smaller than 1 (For example if Keq = 10^-3), then the position of equilibrium is to the left; more reactants are present at equilibrium.

(C) option is correct. If Keq = 1 there will be forward reaction = Backward Reaction

15.

a) Adding H₂O results in more backward reaction so that the equilibrium can be maintained by making more reactants.

b) H₂ removal will again shift the equilibrium in backward direction to produce more H₂ to maintain the equilibrium ration.

c) Adding O₂ shifts the equilibrium in forward direction to produce more products to bring back the equilibrium.

d) Increasing the temperature of an exothermic reaction favors the backward reaction which will result in more H₂ and O_2.