Question

Consider the following exothermic equilibrium system in a closed container. In which direction will the equilibrium shift with each of the disturbances listed below? towards products or reactants or no change?

6H₂O _(l) +  CoCl₄ ^2-_(aq)  ↔ Co(H₂O)₆²⁺_(aq) + 4Cl^- _(aq)

a. adding Na₂CoCl_{4 (aq)}

b. adding Fe(OH)_{3 (s)} .

c. placing it in an ice bath.

d. adding LiCl _(aq) .

e. adding AgNO_{3 (aq)} .

Answer 1

a. adding Na2CoCl4 (aq), shifts the equilibrium towards the right (i.e. towards products)

b. adding Fe(OH)3 (s), shifts the equilibrium towards the right, (i.e towards products). As Fe(OH)3 reacts with Chloride ion to form FeCl3, thus shifts the equilibrium to right

c. placing it in an ice bath.in order to determine shift, the reaction is exothermic or endothermic must be known.

d. adding LiCl (aq) .shifts the equilibrium towards the left (i.e. towards reactants)

e. Adding AgNO3 shifts the equilibrium towards the right (i.e. towards products). As AgNO3 reacts with Chloride ion to form AgCl, thus shifts the equilibrium towards right.