A voltaic cell is constructed from a standardCu²+ Cu half cell (E° red%3D0.337V) and a standardAl³+ |Al half cell (E°red-1.660V).(Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed,leave it blank.)The anode reaction is:Al(s)Al3+(аq)+ЗеThe cathode reaction is:Cu²* (aq)2eCu(s)++The spontaneous cell reaction is:2Al(s)+ 3Cu2* (aq)2A1³*(aq)+ 3Cu2*(aq)The cell voltage is 1.997V.An error has been detected in your answer. Check for typos,miscalculations etc. before submitting your answer.PreviousNext+

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A voltaic cell is constructed from a standard Cu?+ Cu half cell (E° red %3D 0.337V) and a standard Al3+ Al half cell (E° red %D -1.660V). (Use the lowest possible coefficients. Be sure to specify states such as (ag) or (s). If a box is not needed, leave it blank.) The anode reaction is: Al(s) | A1³* (aq) + 3e The cathode reaction is: (aq) 2e Cu(s) + The spontaneous cell reaction is: 3CU2* (aq) | 2A13* (aq) 3CU2*(aq) 13+ 2Al(s) (аq) + + The cell voltage is 1.997 V. An error has been detected in your answer. Check for typos, miscalculations etc. before submitting your answer. Previous Next + +

A voltaic cell is constructed from a standard Cu?+ Cu half cell (E° red %3D 0.337V) and a standard Al3+ Al half cell (E° red %D -1.660V). (Use the lowest possible coefficients. Be sure to specify states such as (ag) or (s). If a box is not needed, leave it blank.) The anode reaction is: Al(s) | A1³* (aq) + 3e The cathode reaction is: (aq) 2e Cu(s) + The spontaneous cell reaction is: 3CU2* (aq) | 2A13* (aq) 3CU2*(aq) 13+ 2Al(s) (аq) + + The cell voltage is 1.997 V. An error has been detected in your answer. Check for typos, miscalculations etc. before submitting your answer. Previous Next + +

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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Similar questions

For each reaction listed, determine its standard cell potential at 25 C and whether the reaction is spontaneous at standard conditions. (a) Mn(s)+Ni2+(aq)Mn2+(aq)+Ni(s) (b) 3Cu2+(aq)+2Al(s)2Al3+(aq)+3Cu(s) (c) Na(s)+LiNO3(aq)NaNO3(aq)+Li(s) (d) Ca(NO3)2(aq)+Ba(s)Ba(NO3)2(aq)+Ca(s)
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?
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.
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+.
Given this reaction, its standard potential, and the standard half-cell potential of 0.34 V for the Cu2+ |Cu half-cell, calculate E° for the Fe(s)|Fe2+(aq) half-cell.
Consider a voltaic cell in which the following reaction occurs. Zn(s)+Sn2+(aq)Zn2+(aq)+Sn(s) (a) Calculate E° for the cell. (b) When the cell operates, what happens to the concentration of Zn2+? The concentration of Sn2+? (c) When the cell voltage drops to zero, what is the ratio of the concentration of Zn2+ to that of Sn2+? (d) If the concentration of both cations is 1.0 M originally, what are the concentrations when the voltage drops to zero?
A half-cell that consists of a copper wire in a 1.00 M Cu(NO3)2 solution is connected by a salt bridge to a solution that is 1.00 M in both Pu3+ and Pu4+, and contains an inert metal electrode. The voltage of the cell is 0.642 V, with the copper as the negative electrode. (a) Write the half-reactions and the overall equation for the spontaneous chemical reaction. (b) Use the standard potential of the copper half-reaction, with the voltage of the cell, to calculate the standard reduction potential for the plutonium half-reaction.
What is the voltage of a concentration cell of Fe2+ ions where the concentrations are 0.0025 and 0.750 M? What is the spontaneous reaction?
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)
From the information provided, use cell notation to describe the following systems: (a) In one half-cell, a solution of Pt(NO3)2 forms Pt metal, while in the other half-Cell, Cu metal goes into a.Cu(NO3)2 solution with all solute concentrations 1 M. (b) The cathode consists of a gold electrode in a 0.55 M Au(NO3)3 solution and the anode is a magnesium electrode in 0.75 M Mg(NO3)2 solution. (c) One half-cell consists of a silver electrode in a 1 M AgNO3 solution, and in the other half-cell, a copper Electrode in 1 M Cu(NO3)2 is oxidized.

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