The standard reduction potential of the permanganate ion, MnO4-, to Mn2+ is 1.51 volt, when it takes place in an acidic aqueous solution. The normal reduction potentials of ions Zn2+, Ag+ and Au+ are, respectively, 0.7618, 0.7992 and 1.692 V (in aqueous solution).Introducing a Pt electrode in a MnO4-/ Mn2+ solution, with a salt bridge, and putting it together with the other electrodes (Zn, Au or Ag) and their aqueous solutions,a) Comment in which case will the permanganate oxide the metalsb) Justify your answerc) In those cases where the oxidation takes place, write the diagram of the celld) Calculate the standard potential of the cells, Eºcell.Result: a) Eºcell >0 d) 0.7108 V, 0.7482 V The standard reduction potential of the permanganate ion, Mn04", to Mn²+ is 1.51 volt,hen it takes place in an acidic aqueous solution. The normal reduction potentials of ions12+, Ag+ and Au+ are, respectively, 0.7618, 0.7992 and 1.692 V (in aqueous solution).troducing a Pt electrode in a MnO4/ Mn²+ solution, with a salt bridge, and putting itgether with the other electrodes (Zn, Au or Ag) and their aqueous solutions,Comment in which case will the permanganate oxide the metalsJustify your answerIn those cases where the oxidation takes place, write the diagram of the cellCalculate the standard potential of the cells, E°cel.1/2esult: a) E°cell >0 d) 0.7108 V, 0.7482 V

Redox potential is a measure of the tendency of a chemical species to get reduced, by accepting…

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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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The standard reduction potential of the permanganate ion, MnO₄^-, to Mn²⁺ is 1.51 volt, when it takes place in an acidic aqueous solution. The normal reduction potentials of ions Zn²⁺, Ag⁺ and Au⁺ are, respectively, 0.7618, 0.7992 and 1.692 V (in aqueous solution).
Introducing a Pt electrode in a MnO₄^-/ Mn²⁺ solution, with a salt bridge, and putting it together with the other electrodes (Zn, Au or Ag) and their aqueous solutions,
a) Comment in which case will the permanganate oxide the metals
b) Justify your answer
c) In those cases where the oxidation takes place, write the diagram of the cell
d) Calculate the standard potential of the cells, Eºcell.

Result: a) Eºcell >0 d) 0.7108 V, 0.7482 V

The standard reduction potential of the permanganate ion, Mn04", to Mn²+ is 1.51 volt,
hen it takes place in an acidic aqueous solution. The normal reduction potentials of ions
12+, Ag+ and Au+ are, respectively, 0.7618, 0.7992 and 1.692 V (in aqueous solution).
troducing a Pt electrode in a MnO4/ Mn²+ solution, with a salt bridge, and putting it
gether with the other electrodes (Zn, Au or Ag) and their aqueous solutions,
Comment in which case will the permanganate oxide the metals
Justify your answer
In those cases where the oxidation takes place, write the diagram of the cell
Calculate the standard potential of the cells, E°cel.
1/2
esult: a) E°cell >0 d) 0.7108 V, 0.7482 V

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