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Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter16: Solubility And Precipitation Equilibria
Section: Chapter Questions
Problem 70AP
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The formation of the iron(III) thiocyanate complex ion is an exothermic equilibrium system. For each change to the system, indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium. An up arrow indicates an increase in concentration, a down arrow indicates a decrease in concentration, and leaving it blank means there is no change in the concentration.

 

increasing the concentration of Fe3+

decreasing the concentration of Fe(SCN)2+

increasing the temperature of the system 

The formation of the iron(III) thiocyanate complex ion is an exothermic equilibrium system. For each change to the system, indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium. An up arrow indicates an increase in concentration, a down arrow indicates a decrease in concentration, and leaving it blank means there is no change in the concentration. Fe3+(aq) + SCN-(aq) = Fe(SCN)²+(aq) increasing the concentration of Fe3+ decreasing the concentration of Fe(SCN)2+ increasing the temperature of the system Answer Bank
Transcribed Image Text:The formation of the iron(III) thiocyanate complex ion is an exothermic equilibrium system. For each change to the system, indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium. An up arrow indicates an increase in concentration, a down arrow indicates a decrease in concentration, and leaving it blank means there is no change in the concentration. Fe3+(aq) + SCN-(aq) = Fe(SCN)²+(aq) increasing the concentration of Fe3+ decreasing the concentration of Fe(SCN)2+ increasing the temperature of the system Answer Bank
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