For the reaction Ag2S <====> 2Ag + S2 what happens to the equilibrium position if aqueous ammonium sulfide is added
A. Shift left
B. Shifts right
C. Does nothing
D. Doubles
E. Halves
does nothing
;eft
To determine the effect of adding aqueous ammonium sulfide on the equilibrium position for the reaction Ag2S <====> 2Ag + S2, we need to consider Le Chatelier's principle.
Le Chatelier's principle states that when a system at equilibrium is subjected to a stress, it will adjust to reduce the effect of that stress and restore equilibrium.
In this case, adding aqueous ammonium sulfide would increase the concentration of sulfide ions (S2-) in the reaction mixture. The sulfide ions are part of the reactant side (Ag2S) of the equilibrium reaction.
According to Le Chatelier's principle, since the concentration of sulfide ions is increased, the system will try to counteract this increase by shifting the equilibrium position in the direction that consumes the excess sulfide ions. In other words, the reaction will shift to the right to use up the additional sulfide ions.
Therefore, the correct answer is:
B. Shifts right
shifts to the left
Ag2S(s) ==> 2Ag^+ + S^2-
(NH4)2S ==> 2NH4^2+ + S^2-
So adding the common ion, S^2-, will shift the equilibrium to the left.