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Chapter 20: Problem 46

The carbon-based reduction method is NOT used for the extraction of [Adv. 2013] (a) Tin from \(\mathrm{SnO}_{2}\) (b) Iron from \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) (c) Aluminium from \(\mathrm{Al}_{2} \mathrm{O}_{3}\) (d) Magnesium from \(\mathrm{MgCO}_{3} \cdot \mathrm{CaCO}_{3}\)

Short Answer

Expert verified
Carbon reduction is not used for aluminium from Al鈧侽鈧�.

Step by step solution

01

Understand Carbon Reduction

The carbon-based reduction method involves reducing metal oxides using carbon (or carbon monoxide) as a reducing agent. This is commonly used for metals such as iron and tin, which form more stable oxides that can be reduced by carbon.
02

Analyze Each Option

Consider each metal given in the options: - Tin (Sn) is reduced from SnO鈧� by carbon. - Iron (Fe) is extracted from Fe鈧侽鈧� using carbon in blast furnaces. - Aluminium (Al) requires electrolysis for extraction from Al鈧侽鈧�, as carbon cannot reduce its oxide. - Magnesium (Mg) is usually extracted from its ores using the electrolysis of molten salts, as it does not reduce with carbon.
03

Identify the Exception

From the analysis, you can see that carbon is not used in the extraction of aluminium from Al鈧侽鈧�. Aluminium has a very stable oxide which carbon cannot reduce, so electrolysis is used instead.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Carbon Reduction Method
The carbon reduction method is a technique in metallurgy used for extracting metals from their oxides. In this method, carbon, often as coke or charcoal, is used as a reducing agent. It works by removing the oxygen from metal oxides and forming carbon dioxide or carbon monoxide. This process is primarily applied to metals like iron and tin. The carbon reacts with the metal oxide, breaking the oxygen bonds and freeing the metal.
For example:
  • The extraction of iron from iron(III) oxide (\( \text{Fe}_2\text{O}_3 \)) uses carbon in a blast furnace, producing iron and carbon dioxide.
  • Tin can be obtained from tin(IV) oxide (\( \text{SnO}_2 \)) using a similar carbon reduction.
However, this method is not applicable for all metals, especially those with very stable metal oxides. Ensure you understand which metals can be reduced using carbon and which require other methods.
Extraction of Metals
Metal extraction involves obtaining metals from their natural mineral deposits. Based on chemical reactivity, different methods are employed to extract a given metal. Metals can either be extracted through:
  • Reduction: Such as the carbon reduction method, suitable for less reactive metals.
  • Electrometallurgy: Using electricity to extract metal from its oxide.
  • Hydrometallurgy: Utilizing aqueous chemistry for metal extraction, common for certain metals.
The appropriate method is selected according to the metal's reactivity and the stability of its compounds. For example, carbon reduction suits iron, but for reactive metals like aluminium and magnesium, more sophisticated methods like electrolysis are necessary.
Aluminium Extraction
Aluminium is extracted from its ore, bauxite, mainly composed of aluminium oxide (\( \text{Al}_2\text{O}_3 \)). Unlike iron or tin, its oxide is too stable for reduction by carbon. Aluminium extraction is achieved through the Bayer process, followed by electrolytic reduction known as the Hall-H茅roult process.
In the Hall-H茅roult process:
  • The purified aluminium oxide is dissolved in molten cryolite.
  • Electricity is passed through this solution, causing redox reactions that split the oxide into pure aluminium and oxygen gas.
This method highlights aluminium's need for electrolysis, given the ineffectiveness of simpler reduction techniques.
Electrolysis
Electrolysis is a chemical process used to drive a non-spontaneous reaction with electricity. It is indispensable in the extraction of highly reactive metals like aluminium and magnesium. This process requires an electrolyte, usually in molten or aqueous form, where the ions can move freely.
In metal extraction, electrolysis works as follows:
  • The positive metal ions migrate to the cathode, where they gain electrons (reduction) and form the pure metal.
  • Simultaneously, at the anode, oxygen is released (oxidation), completing the circuit.
Electrolysis is crucial when oxides are too stable for reduction by carbon, offering a pathway to extract pure metal efficiently. Understanding the principles of electrolysis is key for metallurgy students, especially when dealing with metals that exhibit strong chemical bonds in their oxidized form.

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Most popular questions from this chapter

Match the refining methods (Column I) with metals (Column II).. (I) Liquation (a) \(\mathrm{Zr}\) (II) Zone Refining (b) \(\mathrm{Ni}\) (III) Mond Process (c) Sn (IV) Van Arkel Method (d) Ga (a) (I) \(-(\mathrm{c}) ;(\mathrm{II})-(\mathrm{a}) ;(\mathrm{III})-(\mathrm{b}) ;(\mathrm{IV})-(\mathrm{d})\) (b) (I) - (b); (II) - (c); (III) - (d); (IV) - (a) (c) (I) \(-(\mathrm{c}) ;(\mathrm{II})-(\mathrm{d}) ;(\mathrm{III})-(\mathrm{b}) ;(\mathrm{IV})-(\mathrm{a})\) (d) (I) - (b); (II) - (d); (III) - (a)l (IV) - (c)

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In the electrolysis of alumina, cryolite is added to : (a) lower the melting point of alumina (b) increase the electrical conductivity (c) minimise the anode effect (d) remove imnurities from alumina
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