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Chapter 17: Problem 24

Briefly explain why, for a small anode-tocathode area ratio, the corrosion rate will be higher than for a large ratio.

Short Answer

Expert verified
Answer: The anode-to-cathode area ratio has a significant impact on the corrosion rate. A smaller ratio results in higher corrosion rates due to increased current density and concentrated electron flow, whereas a larger ratio leads to lower corrosion rates with less intense electron flow per unit area.

Step by step solution

01

Understand Anode and Cathode in Corrosion

An anode is an area of a metal surface where corrosion takes place due to the loss of electrons (oxidation). Cathodes, on the other hand, are areas on a metal surface that protect it from corrosion because they attract and consume electrons (reduction). The anode-to-cathode area ratio refers to the relative sizes of an anodic or corroding area (anode) to the nearby protective area (cathode).
02

Examine the Behavior of a Small Anode-to-Cathode Area Ratio

In an electrochemical cell, the anode loses electrons. As the anode-cathode area ratio decreases with a smaller anode area relative to the cathode, the concentration of the electron flow and the corrosion rate will increase. A small ratio has a greater current density (i.e., more electrons flowing per unit area), leading to a more intense corrosion process.
03

Examine the Behavior of a Large Anode-to-Cathode Area Ratio

A large anode-to-cathode area ratio means that the area available for the anode to lose electrons compared to the cathode area increases. Consequently, the current density or electron flow per unit area will be relatively less, leading to a slower corrosion process.
04

Compare Small and Large Ratios

When analyzing the behavior of a small anode-to-cathode area ratio and a large one, we can note that with a small ratio, there is a higher rate of corrosion due to the increased current density or concentrated electron flow. Conversely, a large ratio leads to a lower corrosion rate as electron flow per unit area is less intense.
05

Conclusion

In summary, the corrosion rate will be higher for a small anode-to-cathode area ratio compared to a large one. This is due to the increased current density, which accelerates the corrosion process in a smaller anode area relative to the cathode area.

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Most popular questions from this chapter

For the following pairs of alloys that are coupled in seawater, predict the possibility of corrosion; if corrosion is probable, note which metal/alloy will corrode. (a) Aluminum and cast iron (b) Inconel and nickel (c) Cadmium and zinc (d) Brass and titanium (e) Low-carbon steel and copper

According to Table \(17.3,\) the oxide coating that forms on silver should be nonprotective, and yet Ag does not oxidize appreciably at room temperature and in air. How do you explain this apparent discrepancy?

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

(a) Describe the phenomenon of dynamic equilibrium as it applies to oxidation and reduction electrochemical reactions. (b) What is the exchange current density?

(a) Demonstrate that the CPR is related to the corrosion current density \(i\left(\mathrm{A} / \mathrm{cm}^{2}\right)\) through the expression \\[ \mathrm{CPR}=\frac{K A i}{n \rho} \\] where \(K\) is a constant, \(A\) is the atomic weight of the metal experiencing corrosion, \(n\) is the number of electrons associated with the ionization of each metal atom, and \(\rho\) is the density of the metal. (b) Calculate the value of the constant \(K\) for the CPR in mpy and i in \(\mu A / \mathrm{cm}^{2}\) \(\left(10^{-6} \mathrm{A} / \mathrm{cm}^{2}\right)\)
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