レQuestion 17 of 20へGeneral Chemistry 4th EditionUniversity Sciepresented by MaMcQuarrie Rock GalloglyThe voltage generated by the zinc concentration cell described by the line notationZn(s) Zn*(aq, 0.100 M) || Zn2+(aq, ? M) | Zn(s)is 15.0 mV at 25 °C. Calculate the concentration of the Zn+(aq) ion at the cathode.concentration:Question Source: McQuarrie, Rock, And Gallogly 4e - General ChemsitryPublisi

Lower the value of standard reduction potential, then the given electrode acts as anode and higher the value of standard reduction potential, then the given electrode acts as cathode. a. The anode half reaction (oxidation): Zn(s) --> Zn2+(aq)+ 2e- The cathode half reaction (reduction): Zn2+(aq)+ 2e- - --> Zn(s) The overall cell reaction : Zn(s) + Zn2+(aq, xM) --------> Zn2+(aq, 0.100 M) +Zn(s) E0cell = E0 cathode - E0 anode = -0.74-(-0.74) = 0.0 V Also given emf of the cell, Ecell = 15.0 mV = 15.0 ×10-3 V The cell potential of the cell at 25 degree Celsius at different condition is given by Nernst equation Ecell = E0 cell- (0.05912)log([Zn2+]anode[Zn2+]cathode) 15.0 ×10-3 = 0.0 - (0.05912)log(0.100[Zn2+]cathode) 30.0 ×10-3 = - (0.0591)log(0.100[Zn2+]cathode) [Zn2+]cathode = 0.3218 M Result: The concentration of the Zn2+ion at the cathode = 0.3218 M

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General Chemistry 4th Edition McQuarrie • Rock Gallogly University Sci presented by M The voltage generated by the zinc concentration cell described by the line notation Zn(s) Zn+(aq. 0.100 M) Zn²+(aq, ? M) Zn(s) is 15.0 mV at 25 °C. Calculate the concentration of the Zn+(aq) ion at the cathode. concentration:

General Chemistry 4th Edition McQuarrie • Rock Gallogly University Sci presented by M The voltage generated by the zinc concentration cell described by the line notation Zn(s) Zn+(aq. 0.100 M) Zn²+(aq, ? M) Zn(s) is 15.0 mV at 25 °C. Calculate the concentration of the Zn+(aq) ion at the cathode. concentration:

Chemistry

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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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Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

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