Use the following informa At one of the electrodes of an aluminium-air cell, moist air is bubbled through a sodium hydroxide solution. The half-reaction represented by the equation below occurs. O₂(g) + 2 H₂O(1) + 4e¯→ 4 OH (aq) 17. The other half-reaction involving the aluminium electrode, Al(s), will occur at the i and the type of cell is ii The statement above is completed by the information in row Row A. B. C. D. A. B. i anode anode cathode cathode 18. If the half-reaction given above was assigned a standard reduction potential of zero, then the standard reduction potential of the half-reaction involving the aluminium electrode would be -2.06 V -1.26 V C. +1.26 V D. +2.06 V ii voltaic electrolytic voltaic electrolytic

Use the following informa At one of the electrodes of an aluminium-air cell, moist air is bubbled through a sodium hydroxide solution. The half-reaction represented by the equation below occurs. O₂(g) + 2 H₂O(1) + 4e¯→ 4 OH (aq) 17. The other half-reaction involving the aluminium electrode, Al(s), will occur at the i and the type of cell is ii The statement above is completed by the information in row Row A. B. C. D. A. B. i anode anode cathode cathode 18. If the half-reaction given above was assigned a standard reduction potential of zero, then the standard reduction potential of the half-reaction involving the aluminium electrode would be -2.06 V -1.26 V C. +1.26 V D. +2.06 V ii voltaic electrolytic voltaic electrolytic

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 18.49QE: A half-cell that consists of a copper wire in a 1.00 M Cu(NO3)2 solution is connected by a salt...

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Consider a salt bridge cell in which the anode is a manganese rod immersed in an aqueous solution of manganese(II) sulfate. The cathode is a chromium strip immersed in an aqueous solution of chromium(III) sulfate. Sketch a diagram of the cell, indicating the flow of the current throughout. Write the half-equations for the electrode reactions, the overall equation, and the abbreviated notation for the cell.
Consider a voltaic cell in which the following reaction takes place in basic medium at 25°C. 2NO3-(aq)+3S2(aq)+4H2O3S(s)+2NO(g)+8OH(aq) (a) Calculate E°. (b) Write the Nernst equation for the cell E. (c) Calculate E under the following conditions: PNO=0.994atm,ph=13.7,[S2]=0.154M,[NO3-]=0.472M, .
Determine the standard cell potential and the cell potential under the stated conditions for the electrochemical reactions described here. State whether each is spontaneous or nonspontaueous under each set of conditions at 293.15 K. (a) Hg(l)+S2(aq,0.10M)+2Ag+(aq,0.25M)2Ag(s)+HgS(s) (b) The galvanic cell made from a half-cell consisting of an aluminum electrode in 0.015 M aluminum nitrate solution and a half—cell consisting of a nickel electrode in 025 M nickel(l) nitrate solution. (c) The cell made of a half-cell in which 1.0 M aqueous bromide is oxidized to 0.11 M bromine ion and a half-cell in which aluminum ion at 0.023 M is reduced to aluminum metal. Assume the standard reduction potential for Br2(l) is the same as that of Br2(aq).
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.
The following two half-reactions arc involved in a voltaic cell. At standard conditions, what species is produced at each electrode? Ag++eAgE=0.80VNi2++2eNiE=0.25V
A galvanic cell is based on the following half-reactions at 25C: Ag++eAg H2O2+2H++2e2H2O Predict whether is larger or smaller than for the following cases. a. [Ag+]=1.0M,[H2O2]=2.0M,[H+]=2.0M b. [Ag+]=2.0M,[H2O2]=1.0M,[H+]=1.0107M
A mercury battery, used for hearing aids and electric watches, delivers a constant voltage (1.35 V) for long periods. The half-reactions are HgO(s)+H2O(l)+2eHg(l)+2OH(aq)Zn(s)+2OH(aq)Zn(OH)2(s)+2e Which half-reaction occurs at the anode and which occurs at the cathode? What is the overall cell reaction?
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?
Give the notation for a voltaic cell whose overall cell reaction is Mg(s)+2Ag+(aq)Mg2+(aq)+2Ag(s) What are the half-cell reactions? Label them as anode or cathode reactions. What is the standard cell potential of this cell?
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?
You have 1.0 M solutions of Al(NO3)3 and AgNO3 along with Al and Ag electrodes to construct a voltaic cell. The salt bridge contains a saturated solution of KCl. Complete the picture associated with this problem by a writing the symbols of the elements and ions in the appropriate areas (both solutions and electrodes). b identifying the anode and cathode. c indicating the direction of electron flow through the external circuit. d indicating the cell potential (assume standard conditions, with no current flowing). e writing the appropriate half-reaction under each of the containers. f indicating the direction of ion flow in the salt bridge. g identifying the species undergoing oxidation and reduction. h writing the balanced overall reaction for the cell.
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.