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Consider the following system at equilibrium: Fes (s) = Fe²+ (aq) + S²- (aq) How would the concentrations of Fe2+ and S2- change to reestablish the equilibrium if potassium sulfide, K2S, was added to the system? Fe2* would increase, while s2 decreases. Os2- would increase, while Fe2* decreases. No change in Fe2+, but s2 would decrease The concentration of Fe2* and S2- would remain constant. O Fe2+ would increase, but S2 will not change.

Consider the following system at equilibrium: Fes (s) = Fe²+ (aq) + S²- (aq) How would the concentrations of Fe2+ and S2- change to reestablish the equilibrium if potassium sulfide, K2S, was added to the system? Fe2* would increase, while s2 decreases. Os2- would increase, while Fe2* decreases. No change in Fe2+, but s2 would decrease The concentration of Fe2* and S2- would remain constant. O Fe2+ would increase, but S2 will not change.

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.98PAE
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Consider the following system at equilibrium: FeS (s) = Fe²+ (aq) + S²- (aq) How would the concentrations of Fe2* and s2- change to reestablish the equilibrium if potassium sulfide, K2S, was added to the system? Fe2* would increase, while s2 decreases. Os2- would increase, while Fe2+ decreases. O No change in Fe2*, but s2 would decrease The concentration of Fe2* and s2 would remain constant. O Fe2+ would increase, but S2- will not change.
Transcribed Image Text:Consider the following system at equilibrium: FeS (s) = Fe²+ (aq) + S²- (aq) How would the concentrations of Fe2* and s2- change to reestablish the equilibrium if potassium sulfide, K2S, was added to the system? Fe2* would increase, while s2 decreases. Os2- would increase, while Fe2+ decreases. O No change in Fe2*, but s2 would decrease The concentration of Fe2* and s2 would remain constant. O Fe2+ would increase, but S2- will not change.
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