A standard galvanic cell is constructed with Pb2+ | Pb and Cu2+ | Cut half cell compartments connected by a salt bridge.Which of the following statements are correct?Hint: Refer to a table of standard reduction potentials.(Choose all that apply.)Cu2+ is reduced at the cathode.The cathode compartment is the Cu2+ | Cut compartment.As the cell runs, anions will migrate from the Pb2+ | Pb compartment to the Cu2+ | Cu+ compartment.The cathode compartment is the Pb2+ || Pb compartment.In the external circuit, electrons flow from the Pb2+ | Pb compartment to the Cu2+ | Cut compartment. A standard galvanic cell is constructed in which a Sn2+ | Sn half cell acts as the cathode. Which of the following statementsare correct?Hint: Refer to a table of standard reduction potentials.(Choose all that apply.)The anode compartment could be F2 | F.In the external circuit, electrons flow from the other compartment to the Sn2+ | Sn compartment.The cathode reaction is Sn -> Sn2+ + 2eSn2+ is reduced at the cathode.The cathode reaction is Sn2+ + 2e-> Sn

Defining Galvanic cell:Galvanic cell is a type of electrochemical cell that converts chemical energy…

Answered: A standard galvanic cell is constructed…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 14P

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The mass of three different metal electrodes, each from a different galvanic cell, were determined before and after the current generated by the oxidation-reduction reaction in each cell was allowed to flow for a few minutes. The first metal electrode, given the label A, was found to have increased in mass; the second metal electrode, given the label B, did not change in mass; and the third metal electrode, given the label C, was found to have lost mass. Make an educated guess as to which electrodes were active and which were inert electrodes, and which were anode(s) and which were the cathode(s).
Use the data from the table of standard reduction potentials in Appendix H to calculate the standard potential of the cell based on each of the following reactions. In each case, state whether the reaction proceeds spontaneously as written or spontaneously in the reverse direction under standard-state conditions. (a) H2(g)+Cl2(g)2H+(aq)+2Cl(aq) (b) Al3+(aq)+3Cr2+(aq)Al(s)+3Cr3+(aq) (c) Fe2+(aq)+Ag+(aq)Fe3+(aq)+Ag(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?
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
Diagram the following galvanic cell, indicating the directionof flow of electrons in the external circuit and themotion of ions in the salt bridge. Pt(s)|Cr2+(aq),Cr3+(aq)||Cu2+(aq)|Cu(s) Write a balanced equation for the overall reaction in thiscell.
Is it reasonable to conclude that a potential could be assigned to each half-cell in a voltaic cell, based on these data for three voltaic cells? Explain. Zn(s)|Zn2+(aq)||Cu2+(aq)|Cu(s) cell potential=1.10 V Zn(s)|Zn2+(aq)||Ag+(aq)|Ag(s) cell potential=1.56 V Cu(s)|Cu2+(aq)||Ag+(aq)|Ag(s) cell potential=0.46 V
The standard potential of the cell reaction Ag+(aq)+Eu2+(aq)Ag(s)+Eu3+(aq) is E = +1.23 V. Use the tabulated standard potential of the silver half-reaction to find the standard reduction potential for the europium half-reaction.
Determine the overall reaction and its standard cell potential at 25 C for the reaction involving the galvanic cell in which cadmium metal is oxidized to 1 M cadmium(II) ion and a half—cell consisting of an aluminum electrode in 1 M aluminum nitrate solution. 15 the reaction spontaneous at standard conditions?
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?
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).
Using values from the table of standard reduction potentials, calculate the cell potentials of the following cells. (a) Ga(s)|Ga3+(aq)Ag+(aq)|Ag(s) (b) Zn(s)|Zn2+(aq)Cr3+(aq)|Cr(s) (c) Fe(s),FeS(s)|S2-(aq)Sn2+(aq)|Sn(s)
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)

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