Chapter 17: Problem 20
Briefly describe the phenomenon of passivity. Name two common types of alloy that passivate.
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Chapter 17: Problem 20
Briefly describe the phenomenon of passivity. Name two common types of alloy that passivate.
These are the key concepts you need to understand to accurately answer the question.
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An Fe/Fe \(^{2+}\) concentration cell is constructed in which both electrodes are pure iron. The \(\mathrm{Fe}^{2+}\) concentration for one cell half is \(0.5 M\) and for the other cell half is \(2 \times 10^{-2} M .\) Is a voltage generated between the two cell halves? If so, what is its magnitude and which electrode will be oxidized? If no voltage is produced, explain this result.
An electrochemical cell is constructed such that on one side a pure \(\mathrm{Zn}\) electrode is in contact with a solution containing \(\mathrm{Zn}^{2+}\) ions at a concentration of \(10^{-2} M\). The other cell half consists of a pure Pb electrode immersed in a solution of \(\mathrm{Pb}^{2+}\) ions that has a concentration of \(10^{-4} M\). At what temperature will the potential between the two electrodes be \(+0.568 \mathrm{~V}\) ?
Briefly describe the two techniques that are used for galvanic protection.
Demonstrate the following: (a) the value of \(\mathscr{F}\) in Equation \(17.19\) is \(96,500 \mathrm{C} / \mathrm{mol}\) (b) at \(25^{\circ} \mathrm{C}(298 \mathrm{~K})\), $$ \frac{R T}{n^{-F}} \ln x=\frac{0.0592}{n} \log x $$
For a concentration cell, briefly explain why corrosion occurs at the region having the lower concentration.
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