A voltaic cell is constructed by immersing a strip of silver in a 1.0 M AgNO_3 solution and a...


A voltaic cell is constructed by immersing a strip of silver in a {eq}1.0 \ M \ AgNO_3 {/eq} solution and a strip of cadmium metal in a {eq}1.0 \ M \ Cd(NO_3)_2 {/eq} solution. The circuit is completed by a wire and a salt bridge in the usual way.

(a) What would be the potential of the cell if it was modified to use a {eq}0.10 \ M \ AgNO_3 {/eq} solution and a {eq}0.30 \ M \ Cd(NO_3)_2 {/eq} solution instead?

Nernst Equation:

An electrochemical cell is a device that operates by using some type of overall redox reaction system. At a given set of cell conditions the reaction has a cell potential value in volts. The sign of this value tells you whether the cell is voltaic or electrolytic at these conditions. These conditions may be standard, in which case you have the standard cell potential that is readily computed from the electrochemical series. However, there are also numerous possible sets of non-standard conditions. For example, you could use different molarity values for your redox-active aqueous species. The cell potential changes and we find the new value using the Nernst equation. Sometimes the non-standard conditions can turn a voltaic cell into an electrolytic cell, or vice versa, due to a change in the sign of the cell potential.

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This question involves a voltaic cell consisting of a cadmium anode (oxidation) and a silver cathode (reduction). The overall redox reaction equation...

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Nernst Equation: Example & Calculator
Nernst Equation: Example & Calculator


Chapter 12 / Lesson 5

Learn what the Nernst equation is and see the Nernst equation formula derivation. Learn how to use the Nernst equation and simplified Nernst equation from examples.

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