Ch.20 - Electrochemistry

Problem 87b

Chapter 20, Problem 87b

Determine whether or not each metal, if coated onto iron, would prevent the corrosion of iron. b. Sn

Verified step by step guidance

insert step 1> Determine the standard reduction potentials for both iron (Fe) and tin (Sn) from a standard reduction potential table.

insert step 2> Compare the standard reduction potential of Sn with that of Fe.

insert step 3> Understand that a metal with a higher reduction potential than iron will not prevent corrosion, as it will not act as a sacrificial anode.

insert step 4> Recognize that if Sn has a higher reduction potential than Fe, it will not prevent the corrosion of iron.

insert step 5> Conclude that Sn, if it has a higher reduction potential than Fe, will not protect iron from corrosion.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Corrosion

Corrosion is the process by which metals deteriorate due to chemical reactions with their environment, often involving oxidation. In the case of iron, it typically forms rust (iron oxide) when exposed to moisture and oxygen. Understanding corrosion is essential for determining how different metals can protect iron from this degradation.

Galvanic Protection

Galvanic protection is a method of preventing corrosion by using a more reactive metal to protect a less reactive one. When a more reactive metal, such as zinc, is coated onto iron, it sacrifices itself to corrosion, thereby protecting the iron. This principle is crucial for evaluating whether a metal like tin (Sn) can effectively prevent iron corrosion.

Noble and Reactive Metals

Metals can be classified as noble or reactive based on their tendency to oxidize. Noble metals, such as gold and platinum, resist corrosion, while reactive metals, like zinc and aluminum, corrode more easily. Tin (Sn) is considered a relatively noble metal, and understanding its position in the reactivity series helps assess its effectiveness in protecting iron from corrosion.

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Refer to the tabulated values of ∆G°_f in Appendix IIB to calculate E°_cell for the fuel-cell breathalyzer, which employs the following reaction. ((∆G° for HC₂H₃O₂(g) = -374.2 kJ/mol.)

CH₃CH₂OH(g) + O₂(g) → HC₂H₃O₂(g) + H₂O(g)

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