Question

Some AgNO3, NaCl, and AgCl are added to water and the following reaction consumes some AgCl until equilibrium is established. The temperature and pressure remain constant. Note: AgNO3 and NaCl are highly soluble in water. AgCl has limited solubility in water.

Ag+(aq) + Cl−(aq) ⇌ AgCl(s)

Which of the following conditions must be satisfied: (i) initially; and (ii) at equilibrium?
(i) ΔrG > 0 and Q > K (ii) ΔrG = 0
(i) ΔrG° > 0 and Q > K (ii) ΔrG° = 0
(i) ΔrG > 0 and Q < K (ii) ΔrG = 0
(i) ΔrG° < 0 and Q < K (ii) ΔrG° = 0
(i) ΔrG < 0 and Q < K (ii) ΔrG = 0

Answer 1

i think its (i) ΔrG > 0 and Q > K (ii) ΔrG = 0
pls confirm

Answer 2

I'm sorry but I don't understand the problem. In my mind there is no way that AgCl can be consumed. The solution MUST precipitate more AgCl so AgCl is formed and not consumed. Also, adding AgNO3 and NaCl to a solution that was already at equilibrium with AgCl(s) the MORE AgCl would ppt.