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Chapter 17: Problem 25

For a concentration cell, briefly explain why corrosion occurs at the region having the lower concentration.

Short Answer

Expert verified
Answer: Corrosion occurs at the lower concentration region because this is where the electrode acts as the anode and the oxidation half-cell reaction takes place. This oxidation process results in the loss of metal, releasing ions into the solution and forming a metal oxide on the surface, which leads to corrosion. The potential difference created by the concentration difference drives this oxidation process.

Step by step solution

01

Introduction to Concentration Cells

A concentration cell is a type of electrochemical cell where both electrodes are made of the same material, and the potential difference is due to a difference in ion concentration. The half-cell reactions on both electrodes drive the overall cell reaction.
02

Corrosion in Concentration Cells

Corrosion is the process of metal deterioration due to an electrochemical reaction. In a concentration cell, the difference in the ion concentration across the cell creates an electric potential that drives corrosion reactions on the electrodes.
03

Anodic Region

At the region with a lower concentration, the electrode acts as the anode of the cell. This is where the oxidation half-cell reaction occurs, leading to the release of metal ions into the solution and forming a metal oxide on the surface. The oxidation reaction results in the loss of metal and is responsible for corrosion.
04

Cathodic Region

The region with higher concentration acts as the cathode of the cell. The reduction half-cell reaction takes place at the cathode, where reduction of an oxidizing species like oxygen occurs. This reduction reaction does not cause the loss of metal, so the cathode region remains intact.
05

Reason for Corrosion at Lower Concentration

Corrosion occurs at the lower concentration region because this is where the electrode acts as the anode. The oxidation of the metal electrode releases ions into the solution, causing the loss of metal, which eventually leads to corrosion. The potential difference created by the concentration difference drives this oxidation process.

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Most popular questions from this chapter

(a) Briefly explain the difference between oxidation and reduction electrochemical reactions. (b) Which reaction occurs at the anode and which at the cathode?

A piece of corroded metal alloy plate was found in a submerged ocean vessel. It was estimated that the original area of the plate was \(800 \mathrm{~cm}^{2}\) and that approximately \(7.6 \mathrm{~kg}\) had corroded away during the submersion. Assuming a corrosion penetration rate of \(4 \mathrm{~mm} / \mathrm{yr}\) for this alloy in seawater, estimate the time of submersion in years. The density of the alloy is \(4.5 \mathrm{~g} / \mathrm{cm}^{3}\).

Demonstrate the following: (a) the value of \(\mathscr{F}\) in Equation \(17.19\) is \(96,500 \mathrm{C} / \mathrm{mol}\) (b) at \(25^{\circ} \mathrm{C}(298 \mathrm{~K})\), $$ \frac{R T}{n^{-F}} \ln x=\frac{0.0592}{n} \log x $$

Briefly explain why cold-worked metals are more susceptible to corrosion than non-coldworked metals.

(a) What are inhibitors? (b) What possible mechanisms account for their effectiveness?
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