An electrochemical cell is made by placing an iron electrode in 1.00 L of 0.19 M FeSO4 solution and a copper electrode in 1.00 L of 8.80 × 10-² M CuSO4 solution. Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Half-Reaction Fe²+ (aq) + 2e¯¯ ⇒ Fe(s) Cu²+ (aq) + 2e¯ ⇒ Cu(s) Standard Potential, E° (V) -0.41 = 0.34 a. What is the initial voltage of this cell when it is properly constructed? Initial voltage = b. Calculate the final concentration of Cu²+ in this cell if it is allowed to produce an average current of 1.78 amp for 241 s. Final concentration of Cu²+ M
An electrochemical cell is made by placing an iron electrode in 1.00 L of 0.19 M FeSO4 solution and a copper electrode in 1.00 L of 8.80 × 10-² M CuSO4 solution. Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Half-Reaction Fe²+ (aq) + 2e¯¯ ⇒ Fe(s) Cu²+ (aq) + 2e¯ ⇒ Cu(s) Standard Potential, E° (V) -0.41 = 0.34 a. What is the initial voltage of this cell when it is properly constructed? Initial voltage = b. Calculate the final concentration of Cu²+ in this cell if it is allowed to produce an average current of 1.78 amp for 241 s. Final concentration of Cu²+ M
General Chemistry - Standalone book (MindTap Course List)
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.140QP
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Transcribed Image Text:An electrochemical cell is made by placing an iron electrode in 1.00 L of 0.19 M
FeSO4 solution and a copper electrode in 1.00 L of
8.80 × 10-² M
CuSO4 solution.
Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C
Cathode (Reduction)
Half-Reaction
¯(aq) + 2e¯ ⇒ Fe(s)
Cu²+ (aq) + 2e¯¯ ≈ Cu(s)
Fe²+
Standard
Potential, E° (V)
-0.41
=
0.34
a. What is the initial voltage of this cell when it is properly constructed?
Initial voltage
2+
b. Calculate the final concentration of Cu²+ in this cell if it is allowed to produce an average
current of 1.78 amp for 241 s.
Final concentration of Cu²+
M
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