Corrosion of Metals
Chemistry ⇒ Metals and Non-metals
Corrosion of Metals starts at 8 and continues till grade 12.
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See sample questions for grade 11
A ship's hull is made of iron and is protected from corrosion by attaching blocks of magnesium. Explain why magnesium is used.
Describe one environmental impact of metal corrosion.
Describe the process of cathodic protection in preventing corrosion.
Describe the role of moisture in the corrosion of iron.
Explain why aluminum does not corrode as rapidly as iron, even though it is more reactive.
Explain why copper develops a green patina over time when exposed to air.
Explain why iron nails rust faster in coastal areas than in dry inland areas.
Explain why painting iron objects helps prevent corrosion.
Explain why salt water accelerates the corrosion of iron compared to pure water.
State one reason why stainless steel is more resistant to corrosion than ordinary steel.
What is corrosion? Define the process in your own words.
A pipeline made of iron is buried underground and is found to corrode rapidly in certain areas. Suggest two possible reasons for the variation in corrosion rate along the pipeline and explain your reasoning.
A steel bridge is exposed to acid rain over several years. Describe the chemical reactions that occur during the corrosion process and explain how acid rain accelerates corrosion.
Calculate the mass of iron lost per year from a steel structure if a corrosion current of 0.5 A flows continuously. (Molar mass of Fe = 56 g/mol, 1 Faraday = 96,500 C)
Describe how the use of inhibitors can reduce the rate of corrosion in industrial systems, and give an example of a commonly used inhibitor.
Explain why the corrosion of iron is considered an electrochemical process, and describe the roles of the anode and cathode in this process.
Explain, using electrochemical principles, why connecting iron to copper in the presence of an electrolyte can accelerate the corrosion of iron.
