5. Which of the following statements is TRUE about this equilibrium? Cu(s) + 2Ag+ (aq) → Cu²+ (aq) + 2Ag(s) Keq = 2 X 1015 at 25°C a. If a piece of copper is placed in a solution of excess Ag2+ ions, it's mass will eventually decrease to nearly 0. b. The reactants are favored in this reaction. c. Ag2+ will be in higher concentration than any other components. Silver must be higher on the activity series than copper. d.

Chemistry & Chemical Reactivity
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Chapter19: Principles Of Chemical Reactivity: Electron Transfer Reactions
Section19.8: Counting Electrons
Problem 1RC: 1. If you wish to convert 0.0100 mol of Au3+ (aq) ions into Au(s) in a “gold-plating” process, how...
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5. Which of the following statements is TRUE about this equilibrium?
Cu(s) + 2Ag+ (aq) → Cu²+ (aq) + 2Ag(s)
Keq = 2 X 1015 at 25°C
a. If a piece of copper is placed in a solution of excess Ag²+ ions, it's mass will eventually decrease to
nearly 0.
b.
The reactants are favored in this reaction.
c. Ag2+ will be in higher concentration than any other components.
Silver must be higher on the activity series than copper.
d.
Transcribed Image Text:5. Which of the following statements is TRUE about this equilibrium? Cu(s) + 2Ag+ (aq) → Cu²+ (aq) + 2Ag(s) Keq = 2 X 1015 at 25°C a. If a piece of copper is placed in a solution of excess Ag²+ ions, it's mass will eventually decrease to nearly 0. b. The reactants are favored in this reaction. c. Ag2+ will be in higher concentration than any other components. Silver must be higher on the activity series than copper. d.
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