91/1 pointIf a standard Cu|Cu2+ electrode is connected to a standard Al|A13+ electrode, which of the following is true?Al3+ is oxidizedCu is oxidized● Al is oxidizedCu2+ is oxidized

Step 1: From the table of standard reduction potentials, find the reduction half-reactions and their…

Answered: 9 1/1 point If a standard Cu|Cu2+…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 120AE

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Calculate the cell potential of a cell operating with the following reaction at 25C, in which [MnO4] = 0.010 M, [Br] = 0.010 M. [Mn2] = 0.15 M, and [H] = 1.0 M. 2MNO4(aq)+10Br(aq)+16H+(aq)2MN2(aq)+5Br2(l)+8H2O(l)
An electrochemical cell is set up using the following unbalanced reaction: Ma+(aq)+N(s)N2+(aq)+M(s) The standard reduction potentials are: The cell contains 0.10 M N2+ and produces a voltage of 0.180 V. If the concentration of Ma+ is such that the value of the reaction quotient Q is 9.32 103, calculate [Ma+]. Calculate wmax for this electrochemical cell.
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.
An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?
The standard potential for the reduction of AgSCN is 0.0895 V. AgSCN(s)+eAg(s)+SCN(aq) Find another electrode potential to use together with the above value and calculate Kspfor AgSCN.
Consider a galvanic cell based on the following half-reactions: a. What is the expected cell potential with all components in their standard states? b. What is the oxidizing agent in the overall cell reaction? c. What substances make up the anode compartment? d. In the standard cell, in which direction do the electrons flow? e. How many electrons are transferred per unit of cell reaction? f. If this cell is set up at 25C with [Fe2+] = 2.00 104 M and [La3+] = 3.00 103 M, what is the expected cell potential?
An electrochemical cell consists of a silver metal electrode immersed in a solution with [Ag+] = 1.0 M separated by a porous disk from a copper metal electrode. If the copper electrode is placed in a solution of 5.0 M NH3 that is also 0.010 M in Cu(NH3)42+, what is the cell potential at 25C? Cu2+(aq)+4NH3(aq)Cu(NH3)42+(aq)K=1.01013
Given the following two standard reduction potentials, solve for the standard reduction potential of the half-reaction M3++eM2+ (Hint: You must use the extensive property G to determine the standard reduction potential.)
Consider a galvanic cell based on the following half-reactions: a. What is the standard potential for this cell? b. A nonstandard cell is set up at 25C with [Mg2+] = 1.00 105 M. The cell potential is observed to be 4.01 V. Calculate [Au3+] in this cell.
An electrochemical cell consists of a nickel metal electrode immersed in a solution with [Ni2+] = 1.0 M separated by a porous disk from an aluminum metal electrode. a. What is the potential of this cell at 25C if the aluminum electrode is placed in a solution in which [Al3+] = 7.2 103 M? b. When the aluminum electrode is placed in a certain solution in which [Al3+] is unknown, the measured cell potential at 25C is 1.62 V. Calculate [Al3+] in the unknown solution. (Assume Al is oxidized.)

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9 1/1 point If a standard Cu|Cu2+ electrode is connected to a standard Al|A13+ electrode, which of the following is true? Al3+ is oxidized Cu is oxidized ● Al is oxidized Cu2+ is oxidized