(0.43 M) as the anode and the half-cell Sn2+(x M) | Sn(s) as the cathode; the measured cell voltage was 0.52 V. Calculate x, the molarity of Sn2+ in the cathode. (Please show work written out step by step on paper)

(0.43 M) as the anode and the half-cell Sn2+(x M) | Sn(s) as the cathode; the measured cell voltage was 0.52 V. Calculate x, the molarity of Sn2+ in the cathode. (Please show work written out step by step on paper)

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 77AP

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Concept explainers

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.

Question

A voltaic cell was constructed using the half-cell Cr(s) | Cr3+
(0.43 M) as the anode and the half-cell Sn2+(x M) | Sn(s) as
the cathode; the measured cell voltage was 0.52 V. Calculate
x, the molarity of Sn2+ in the cathode. (Please show work
written out step by step on paper)

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