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A voltaic cell that uses the reaction

PdCl42- (aq) + Cd(s) → Pd(s) + 4 Cl-(aq) + Cd2+(aq), has a measured standard cell potential of +1.03 V. (a) Write the two half-cell reactions. (b) By using data from Appendix E, determine E° red for the reaction involving Pd. (c) Sketch the voltaic cell, label the anode and cathode, and indicate the direction of electron flow.

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Keith Leannon
Keith LeannonLv2
29 May 2020

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Related questions

Voltaic cell that uses the reaction

T13+(aq) + 2Cr2+(aq)→T1+(aq) + 2Cr3+(aq), has a measured standard cell potential of +1.19 V.

(a) Write the two half-cell reactions. (b) By using data from Appendix E, determine E°red for the reduction of T13+(aq) to T1+(aq).

(c) Sketch the voltaic cell, label the anode and cathode, and indicate the direction of electron flow.

OK, I am getting a bit dis-inchanted with this site. Thisquestion has been asked several times and there appaer to be twodifferent answer and no clear answer on who is right. (One responsesays the answer is wrong)

Please clarifiy,

Use the following voltaic cell reaction;

PdCl4(aq)+Cd(s)--> Pd(s) + 4 Cl^-(aq) + Cd^2-(aq) E cell=+1.03V

a) half reactions

b) Calcutlate E red involving Pd

c) ID the anode and cathode


Martin

Sketch a voltaic cell for this redox reaction: Ni2+(aq) + Mg (s) ----> Ni (s) + Mg2+(aq)

a.Label the anode and cathode.

b.Write the half reactions.

c.Indicate the direction of electron flow.

d.Calculate Eocell.

e.Write the line notation for the cell.

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