Consider the following reaction: 2CrO4-2(aq) + 2H+(aq) <--> Cr2O7-2(aq) + H2O(l) K = 3.13 x 104 [yellow] [orange] This equilibrium can be disturbed by altering different factors, such as ion concentrations or temperature, and by the addition of other stances to the system.
Consider the following reaction: 2CrO4-2(aq) + 2H+(aq) <--> Cr2O7-2(aq) + H2O(l) K = 3.13 x 104 [yellow] [orange] This equilibrium can be disturbed by altering different factors, such as ion concentrations or temperature, and by the addition of other stances to the system.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter14: Acids And Bases
Section14.9: Lewis Acids And Bases
Problem 14.26E
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Before they were known to a carcinogen (a cancer-causing agent), chromium ions were often used in equilibrium demonstrations because polyatomic ions of chromium and oxygen exist in multiple colours, making shifts in equilibrium easy to observe. Consider the following reaction:
2CrO4-2(aq) + 2H+(aq) <--> Cr2O7-2(aq) + H2O(l)
K = 3.13 x 104 [yellow] [orange]
This equilibrium can be disturbed by altering different factors, such as ion concentrations or temperature, and by the addition of other stances to the system.
a. If the temperature of this system is increased, the solution turns from orange to yellow. Explain how that shift in equilibrium can be explain using the enthalpy of the reaction.
b. Aqueous ammonia, NH3, is added to the solution and the colour becomes an intense yellow. Explain why that shift in equilibrium occurs in this reaction.
c.If 0.015 M concentrations of all species are placed in a reaction vessel and allowed to react, what will the equilibrium concentrations be for each species?
d. If you were to place 0.12 M concentrations of each species into a reaction vessel, is the system at equilibrium? How do you know?
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