A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction:3Cu2* (ag) +2A1 (s) –- 3Cu (s) + 2AI³* (aq)2+in one half-cell and 4.12 M Al" in the other.3+Suppose the cell is prepared with 3.11 M CuCalculate the cell voltage under these conditions. Round your answer to 3 significant digits.

Answered: Image /qna-images/answer/fdde834b-375c-40fb-92e1-0f57871c2b78.jpg

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3Cu* (aq)+2A1 (s) → 3Cu (s) +2AI* (aq) 2+ Suppose the cell is prepared with 3.11 M Cu in one half-cell and 4.12 M AlI" in the other. 13+ Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. x10 ロロ

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3Cu* (aq)+2A1 (s) → 3Cu (s) +2AI* (aq) 2+ Suppose the cell is prepared with 3.11 M Cu in one half-cell and 4.12 M AlI" in the other. 13+ Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. x10 ロロ

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter19: Applications Of Standard Electrode Potentials

Section: Chapter Questions

Problem 19.8QAP

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Similar questions

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The half-cells Ag+(aq. 1.0 M)|Ag(s) and H+(aq, ? M)|H2(1.0 bar) are linked by a salt bridge to create a voltaic cell. With the silver electrode as the cathode, a value of 0.902 V is recorded tor kcell at 298 K. Determine the concentration of H+ and the pH of the solution.
An electrolysis experiment is performed to determine the value of the Faraday constant (number of coulombs per mole of electrons). In this experiment, 28.8 g of gold is plated out from a AuCN solution by running an electrolytic cell for two hours with a current of 2.00 A. What is the experimental value obtained for the Faraday Constant?
A galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.
Assume the following electrochemical cell simulates the galvanic cell formed by copper and zinc in seawater at pH 7.90 and 25 C. Zn | Zn(OH)2(s) | OH(aq) || Cu(OH)2(s) | Cu(s) a. Write a balanced equation for the reaction that occurs at the cathode. b. Write a balanced equation for the reaction that occurs at the anode. c. Write a balanced chemical equation for the overall reaction. d. Determine the potential (in volts) of the cell.
It took 150. s for a current of 1.25 A to plate out 0.109 g of a metal from a solution containing its cations. Show that it is not possible for the cations to have a charge of 1+.
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