Extraction of Metals from Ores

Chemistry ⇒ Metals and Non-metals

Extraction of Metals from Ores starts at 9 and continues till grade 12. QuestionsToday has an evolving set of questions to continuously challenge students so that their knowledge grows in Extraction of Metals from Ores. How you perform is determined by your score and the time you take. When you play a quiz, your answers are evaluated in concept instead of actual words and definitions used.

See sample questions for grade 12

A sample of iron ore contains 60% Fe₂O₃. Calculate the mass of pure iron that can be obtained from 100 kg of this ore. (Atomic masses: Fe = 56, O = 16)

Describe the difference between calcination and roasting.

Describe the process of froth flotation used in the concentration of ores.

Describe the role of coke in the extraction of iron from its ore in the blast furnace.

Explain the term 'gangue' in metallurgy.

Explain why carbon cannot be used to reduce aluminium oxide to aluminium.

Explain why gold and platinum are found in a free state in nature.

Explain why highly reactive metals are extracted by electrolysis of their molten salts.

Name the chief ore of iron used in the extraction of iron.

Name the process used to extract copper from its sulphide ore.

Name the process used to purify copper after extraction from its ore.

State the purpose of adding cryolite in the extraction of aluminium by electrolysis.

State the reason why flux is added during the extraction of metals from ores.

A sample of chalcopyrite (CuFeS₂) weighing 200 g is processed for copper extraction. If the overall efficiency of copper recovery is 80%, calculate the mass of copper obtained. (Atomic masses: Cu = 63.5, Fe = 56, S = 32)

Consider the following scenario: A metallurgist is extracting a metal from its oxide ore using hydrogen gas as the reducing agent. The metal obtained is found to be contaminated with hydrogen. Suggest a method to obtain pure metal and explain the principle behind it.

During the extraction of silver by the cyanide process, the addition of zinc leads to the precipitation of silver. Write the balanced chemical equation for this reaction and explain the role of zinc.

Explain why the extraction of metals at the top of the reactivity series (such as potassium and sodium) is always carried out by electrolysis of their molten salts and not by chemical reduction methods.

Explain, with relevant chemical equations, why the extraction of zinc from zinc blende (ZnS) involves both roasting and reduction steps, whereas the extraction of iron from hematite (Fe₂O₃) does not require roasting.