GCSE Chemistry - What is Corrosion and How to Stop it #71

The video tutorial explores the concept of corrosion, focusing on rusting, a type of corrosion where iron reacts with oxygen and water to form rust. It explains the redox reaction involved in rusting and the conditions necessary for it to occur. The tutorial also compares how different metals like iron and aluminum corrode, highlighting the protective layer formed by aluminum oxide. Finally, it discusses methods to prevent rusting, including barrier methods like painting and electroplating, and sacrificial methods such as galvanizing with zinc.

What type of reaction is involved in the rusting of iron?

• Combustion reaction

• Synthesis reaction

• Redox reaction

• Decomposition reaction

Which two elements must be present for rusting to occur?

• Iron and nitrogen

• Oxygen and hydrogen

• Oxygen and water

• Iron and carbon dioxide

In the test tube experiment, which test tube will show rusting?

• The one with both oxygen and water

• The one with only water

• None of them

• The one with only oxygen

Why does aluminum not corrode like iron?

• It is a non-reactive metal

• It forms a protective layer of aluminum oxide

• It reacts with water instead

• It is not exposed to oxygen

What is the purpose of painting iron surfaces?

• To increase their weight

• To make them conduct electricity

• To prevent them from rusting

• To make them look attractive

How does the sacrificial method prevent rusting?

• By painting the iron surface

• By covering iron with a non-reactive metal

• By using a more reactive metal to oxidize first

• By keeping iron away from water

What is galvanizing?

• Painting iron with oil

• Electroplating iron with copper

• Covering iron with plastic

• Coating iron with zinc