CBSE Class 12 Chemistry General Principles Process of Isolation of Elements Questions

SA (I) QUESTIONS (2 - MARK QUESTIONS)

22. What is hydrometallurgy? Give one example where it is used for metal extraction.
[Ans. : Leaching followed by reduction is called hydrometallurgy. It is used in extraction and copper

23. Name the process for the benefaction/concentration of (i) an ore having lighter impurities (ii) sulphide ore.

24. Mention the role of cryolite in the extraction of aluminium.

25. Mention the role of following :
(a) SiO₂ in the metallurgy of Cu.
(b) CaCO₃ in the metallurgy of Fe.
(c) CO in the metallergy of iron
(d) I₂ in the purification of zirconium.

26. Extraction of copper directly from sulphide ore is less favourable than from its oxide through reduction. Explain.
[Ans. : 2Cu S(s) + C(s) → CS₂ (l) + 2Cu(s)
CuO(s) + C(s) → CO (g) + Cu(s)
ΔG value is more –ve in second case as compared with first case]

27. The graphite electrodes in the extraction of ‘alluminium’ by Hall-Heroult process need to be changed frequently. Why?

28. Write the chemical formulae of the following ores (a) Haematite (b) Magnetite (c) Limonite (d) Siderite.
[Ans. : (a) Fe₂O₃ (b) Fe₃O₄ (c) Fe₂O₃.2H₂O (d) FeCO₃]

29. Give equations for the industrial extraction of zinc from calamine.
[Ans. : ZnCO₃ → ZnO + CO₂ (Calcination) ZnO + C → Zn + CO (Reduction)]

30. Name the elements present in anode mud during refining of copper. Why does it contain such elements?
[Ans. : Au and Ag. They are not oxidised at anode. They are less electropositive than copper.]

31. Write the Chemical reactions taking place in different zones in the blast furnace for the extraction of iron from its ore.

32. How are impurities separated from bauxite ore to get pure alumina?

33. Why is the reduction of a metal oxide easier if metal formed is in liquid state at the temperature of reduction?
[Hint : Entropy is more positive when the metal is in liquid state as compared with solid state, so ΔG becomes more –ve]

34. What is pyrometallurgy? Explain with one example.
[Ans. : A process of reducing a metal oxide by heating with either coke or some other reducing agent e.g., Al, Mg etc.
ZnO + C  975k_→ Zn + CO]

35. Write the method to produce Copper matte from copper pyrites.

*38. Copper can be extracted by hydrometallurgy but not zinc. Explain why?
[Hint : E^Ø Zn²⁺/Zn is - ve, E^Ø cu²⁺/cu is + ve]

39. Gibbs energies of formation Δ_fG of MgO(s) and CO(g) at 1273K and 2273 K are given below:
Δ_fG [MgO(s)] = –941 kJ mol^–1 at 1273 K.
Δ_fG [CO(g)] = –439 kJ mol^–1 at 1273 K.
Δ_fG [MgO(s)] = –314 kJ mol^–1 at 2273 K.
Δ_fG [CO(g)] = –628 kJ mol^–1 at 2273 K. 
On the basis of above data, predict the temperature at which carbon can be used as a reducing agent for MgO(s).
[Ans. : For the reaction, MgO(s) + C(s) → Mg(s) + CO(g)
At 1273K, ΔrG = ΔfG[CO(g)] – ΔfG[MgO(s)] = –439 – (–941) KJ mol^–1 = 502 kJ mol^–1
At 2273 K, ΔrG = –628 – (–314) kJ mol^–1 = –314 kJ mol^–1
The temperature is 2273 K]

SA (II) TYPE QUESTIONS (3 - MARK QUESTIONS)

40. State the principles of refining of metal by the following methods.
(a) Zone refining (b) Electrolytic refining (c) Vapour phase refining.

41. How is pure copper obtained from its principle ore? Write the chemical reactions occurring during the extraction.

42. Name the method of refining of the following metals –
(a) Hg (b) Sn (c) Cu (d) Ge (e) Ni (f) Zr
[Ans. : (a) Distillation,
(b) Liquation;
(c) Electrolytic refining
(d) Zone refining;
(e) Mond Process
(f) Van Arkel Processl]

44. The native silver forms a water soluble compound (B) with dilute aqueous solution of NaCN in the presence of a gas (A). The silver metal is obtained by the addition of a metal (C) to (B) and complex (D) is formed as a byproduct. Write the structures of (C) and (D) and identify (A) and (B) in the following sequence – Ag + NaCN + [A] + H2O → [B] + OH– + Na+.
[C] + [B] → [D] + Ag.
[Ans. : [A] = O₂
[B] = Na [Ag(CN)2]
[C] = Zn
[D] = Na2 [Zn (CN)4] ].

45. In the cynamide extraction process of silver pon argentite ore, name the oxidising and reducing agents. Write the chemical equations of the reactions involved.