Corrosion and Its Prevention
Chemistry ⇒ Redox Reactions and Electrochemistry
Corrosion and Its Prevention starts at 12 and continues till grade 12.
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A piece of iron is placed in a solution containing both Cu²⁺ and Zn²⁺ ions. Which metal will deposit on the iron surface, and why?
A ship's hull is protected from corrosion by attaching blocks of zinc. What is the role of zinc in this case?
A steel bridge is exposed to a marine environment. Suggest two methods to prevent its corrosion and explain how they work.
A steel water tank is coated with a layer of zinc. If the zinc layer is damaged, will the steel underneath corrode? Explain your answer.
Calculate the cell potential for the corrosion of iron in acidic medium, given: Fe²⁺ + 2e⁻ → Fe (E° = -0.44 V), O₂ + 4H⁺ + 4e⁻ → 2H₂O (E° = +1.23 V).
Describe the role of electrolytes in the corrosion of metals.
Explain the difference between dry corrosion and wet corrosion.
Explain the term 'passivation' in the context of corrosion.
Explain why aluminum does not corrode as rapidly as iron, even though it is more reactive.
Explain why iron corrodes faster in the presence of dissolved salts.
Explain why iron corrodes more rapidly in the presence of both oxygen and water than in dry air.
Explain why painting a metal surface prevents corrosion.
A buried iron pipeline is protected from corrosion by connecting it to a more reactive metal. Name this method and explain, using electrochemical principles, why it is effective.
A steel structure is exposed to an industrial environment containing SO2 gas. Predict and explain the effect of SO2 on the rate of corrosion of the steel.
Calculate the standard cell potential (E0cell) for the corrosion of zinc in acidic medium, given the following standard reduction potentials:
Zn2+ + 2e− → Zn (E0 = −0.76 V)
O2 + 4H+ + 4e− → 2H2O (E0 = +1.23 V)
Explain why the corrosion of iron is considered an electrochemical process, and describe the roles of anode, cathode, and electrolyte in this process.
Explain, with relevant half-cell reactions, how the presence of both oxygen and carbon dioxide in water accelerates the corrosion of iron compared to water containing only oxygen.
