CBSE Class 12 Chemistry Metallurgy Important Questions and Answers

UNIT – 1 
METALLURGY

 
1. What is the difference between minerals and ores?
 
UNIT – 1 METALLURGY
 
2. What are the various steps involved in extraction of pure metals from their ores?
Steps involved in extraction of pure metals from their ores are
i) Concentration of the ore
ii) Extraction of the crude metal.
iii) Refining of the crude metal.
 
3. What is the role of Limestone in the extraction of Iron from its oxide Fe2O3?
Lime stone (CaO3) is used as a basic flux in the extraction of iron from its oxide Fe2O3.
Limestone decomposes to form CaO
UNIT – 1 METALLURGY Reaction
Impurity silica (SiO2)react with CaOform fusible slagcalcium silicate.
CaO(s) + SiO2(s)→CaSiO3(s)
Flux    Gaugue   Slag
 
4. Which type of ores can be concentrated by froth flotation method? Give two examples for such ores.
Sulphide ores can be concentrated by froth flotation method.
(eg) Galena (PbS), Zinc blende (ZnS)
 
5. Out of coke and CO, which is better reducing agent for the reduction of ZnO? Why?
UNIT – 1 METALLURGY2

Out of coke and CO, coke is better reducing agent than CO for the reduction of ZnO.
ZnO(s)+C →Zn(s)+ CO(g)
In Ellingham diagram formation ZnO line lies above the formation C→CO at low temperature (T1), ZnO line also lies above the CO → CO2 but at high temperature.
 
Hence carbon can be used as a better reducing agent than CO for the reduction of ZnO. Below the temperature T1 both Coke and COcannot reduce ZnO
 
6. Describe a method for refining nickel.
Impure nickel is heated in a stream of carbon monoxide at around 350K. Nickel reacts with CO to form a highly volatile nickel tetracarbonyl. The solid impurities are left behind.
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On heating nickel tetra carbonyl around 460K, decomposes to give pure nickel.
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7. Explain zone refining process with an example
      The principle is fractional crystallisation.
• When an impure metal is melted and allowed to solidify, the impurities will prefer to remain in the molten region. Impurities are more soluble in the melt than in the solid state metal.
• In this process the impure metal is taken in the form of a rod. One end of the rod is heated using a mobile induction heater, melting the metal on that portion of the rod.
• When the heater is slowly moved to the other end pure metal crystallises while impurities will move on to the adjacent molten zone formed due to the movement of the heater.
• As the heater moves further away, the molten zone containing impurities also moves along with it.
• This process is repeated several times by moving the heater in the same direction again and again to achieve the desired purity level.
• This process is carried out in an inert gas atmosphere to prevent the oxidation of metals.
• Germanium, Silicon and Gallium which are used as semiconductor are refined by this process.
 
8. Using the Ellingham diagram given below. 

(A) Predict the conditions under which
i) Aluminium might be expected to reduce magnesia.
ii) Magnesium could alumina.
B) Carbon monoxide is more effective reducing agent than carbon below 983K but, above this temperature, the reverse is true - Explain.
C) It is possible to reduce Fe2O3 by coke at a temperature around 1200K
UNIT – 1 METALLURGY3
A) i) Ellingham diagram for the formation of Al2O3 and MgO intersects around 1600K.
Above this temperature aluminium line lies below the magnesium line. Hence we can use aluminium to reduce magnesia above 1600K.
ii) In Ellingham diagram below 1600K magnesium line lies below aluminium line. Hence below 1600K magnesium can reduce alumina.
UNIT – 1 METALLURGY4
 
B) The two lines for CO→CO2 and C →CO cross at about 983K. Below this temperature the reaction to form CO2 is energetically more favourable hence CO is more effective reducing agent than carbon. But above 983K the formation of CO is preferred, hence carbon is more effective reducing agent than CO above this temperature.
C)In Ellingham diagram above 1000K carbon line lies below the iron line. Hence it is possible to reduce Fe2O3 by coke at a temperature around 1200K.
 
9. Give uses of zinc.
1. Metallic zinc is used in galvanisation to protect iron and steel structures from rusting and corrosion.
2. Zinc is used to produce die - castings in the automobile, electrical and hardware industries.
3. Zinc oxide is used in the manufacture of paints, rubber, cosmetics, pharmaceuticals, plastics, inks, batteries, textiles and electrical equipment.
4. Zinc sulphide is used in making luminous paints, fluorescent lights and x - ray screens.
5. Brass an alloy of zinc is used in water valves and communication equipment as it is highly resistant to corrosion
 
10. Explain the electrometallurgy of aluminium.
Hall – Herold Process
Cathode: Iron tanked lined with carbon
Anode: Carbon blocks
Electrolyte: 20% solution of alumina obtained from bauxite + Molten Cryolite +
                 10% calcium chloride (lowers the melting point of the mixture)
Temperature: Above 1270K
Ionisation of Alumina   Al2O3→ 2Al3+ + 3O2-
Reaction at cathode:   2Al3+(melt) + 6e→2Al(l)
Reaction at anode:     6O2- (melt) →3O2 + 12e
Since carbon acts as anode the following reaction also takes place on it.
C(s) + O2− (melt) → CO + 2e
C(s) + 2O2− (melt) → CO2 + 4e
During electrolysis anodes are slowly consumed due to the above two reactions. Pure aluminium is formed at the cathode and settles at the bottom.
Net electrolysis reaction is
4Al3+ (melt) + 6O2- (melt) + 3C(s)→4Al(l) + 3CO2(g)
 
11. Explain the following terms with suitable examples. i) Gangue ii) Slag
i) Gangue:
The non metallic impurities, rocky materials and siliceous matter present in the ores are called gangue. (eg): SiO2 is the gangue present in the iron ore Fe2O3 .
 
ii) Slag: Slag is a fusible chemical substance formed by the reaction of gangue with a flux.
CaO(s)+ SiO2(s)→CaSiO3(s)
Flux   gangue   slag
 
12. Give the basic requirement for vapour phase refining.
The metal is treated with a suitable reagent to form a volatile compound.
 
Then the volatile compound is decomposed to give the pure metal at high temperature.
 
13. Describe the role of the following in the process mentioned.
i) Silica in the extraction of copper.
ii) Cryolite in the extraction of aluminium.
iii) Iodine in the refining of Zirconium.
iv) Sodium cyanide in froth floatation.
i) In the extraction of copper, silica acts as an acidic flux to remove FeO as slag FeSiO3.
FeO(s) + SiO2(s)→ FeSiO3(s)
             Flux      Slag
ii) As Al2O3 is a poor conductor, cryolite improves the electrical conductivity.
In addition, cryolite serves as an added impurity and lowers the melting point of the electrolyte.
iii) First Iodine forms a Volatile tetraiodide with impure metal, which decomposes to give pure metal. Impure zirconium metal is heated in an evacuated vessel with iodine to form the volatile zirconium tetraiodide (ZrI4). The impurities are left behind, as they do not react with iodine.
 
Zr(s) + 2I2(s)→ZrI4(Vapour)
On passing volatile zirconium tetraiodide vapour over a tungsten filament, it is decomposed to give pure zirconium.
ZrI4(Vapour)→ Zr(s) + 2I2(s)
iv) Sodium cyanide acts as a depressing agent in froth floatation process. When a sulphide ore of a metal contains other metal sulphides, the depressing agent sodium cyanide selectively prevent other metal sulphides coming to the froth. eg: NaCN depresses the floatation property ZnS present in Galena (PbS) by forming a layer of Zinc complex Na2 [Zn(CN)4]on the surface of Zinc sulphide.
 
14. Explain the principle of electrolytic refining with an example.
Crude metal is refined by electrolysis carried out in an electrolytic cell.
Cathode: Thin strips of pure metal.
Anode: Impure metal to be refined.
Electrolyte: Aqueous solution of the salt of the metal with dilute acid.
As current is passed, the metal of interest dissolves from the anode and pass into the electrolytic solution.
At the same time same amount of metal ions from the electrolytic solution will be deposited at the cathode.
Less electro positive impurities in the anode settle down as anode mud.
eg : Electro refining of silver:
Cathode: Pure silver
Anode: Impure silver rods.
 
Electrolyte: Acidified aqueous solution of silver nitrate.
When current passed, the following reactions will take place.
Reaction at anode: Ag(s)→ Ag+(aq) + e
Reaction at cathode: Ag+(aq) + e→ Ag(s)
At anode silver atoms lose electrons and enter the solution. From the solution, silver ions (Ag+)migrate towards the cathode. At cathode silver ions get discharged by gaining electrons and deposited on the cathode.
 
15. The selection of reducing agent depends on the thermodynamic factor: Explain with an example.
• A suitable reducing agent is selected based on the thermodynamic considerations.
• For a spontaneous reaction ΔG should be negative.
 
• Thermodynamically, the reduction of metal oxide with a given reducing agent can occur if ΔG for the coupled reaction is negative.
• Hence the reducing agent is selected in such a way that it provides a large negative ΔG value for the coupled reaction.
• Ellingham diagram is used to predict thremodynamic feasibility of reduction of oxides of one metal by another metal.
• Any metal can reduce the oxides of other metals that are located above it in the diagram.
• Ellingham diagram for the formation of FeO and CO intersects around 1000K. Below this temperature the carbon line lies above the iron line.
• Hence FeO is more stable than CO and the reduction is not thermodynamically feasible.
• However above 1000K carbon line lies below the iron line. Hence at this condition FeO is less stable than CO and the reduction is thermodynamically feasible. So coke can be used as a reducing agent above this temperature.
• Following free energy calculation also confirm that the reduction is thermodynamically favoured.
From the Ellingham diagram at 1500K
2Fe(s)+O2(g)→ 2FeO(g) ΔG1 = − 350 kJmol-1 ............1
2C(s) + O2(g)→ 2CO(g) ΔG2 = − 480 kJmol-1 ............2
Reverse the reaction 1
2FeO(s)→ 2Fe(s) + O2(g)ΔG1 = 350 kJmol-1 ............3
Couple the reactions 2 and 3
2FeO(s)+2C(s)→2Fe(s) + 2CO(g)ΔG3 = − 130 kJmol-1 ............4
• The standard free energy change for the reduction of one mole of FeO is
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16. Give the limitations of Ellingham diagram.
Ellingham diagram is constructed based only on thermodynamic considerations.
1. It gives information about the thermodynamic feasibility of a reaction.
2. It does not tell anything about the rate of the reaction.
3. More over it does not give any idea about the possibility of other reactions that might be taking place.
4. The interpretation of ΔG is based on the assumption that the reactants are in equilibrium with the product which is not always true.
 
17. Write a short note on electrochemical principles of metallurgy.
• Reduction of oxides of active metals such as sodium, potassium etc. by carbon is thermodynamically not feasible.
• Such metals are extracted from their ores by using electrochemical methods.
• In this method the metal salts are taken in fused form or in solution form.
• The metal ion present can be reduced by treating the solution with suitable reducing agent or by electrolysis.
• Gibbs free energy change for the electrolysis is
ΔGo = - nFEo
n = number of electrons involved in the reduction
F = Faraday = 96500 coulombs
Eo = electrode potential of the redox couple.
• If Eo is positive, ΔGo is negative and the reduction is spontaneous.
• Hence a redox reaction is planned in such a way that the e.m.f of the net redox reaction is positive.
• A more reactive metal displaces a less reactive metal from its salt solution.
eg: Cu2+(aq) + Zn(s)→ Cu(s) + Zn2+(aq)
• Zinc is more reactive than copper and displaces copper from its salt solution.
 
II. Evaluate yourself
1. Write the equation for the extraction of silver by leaching with sodium cyanide and show that the leaching process is a redox reaction.
In the metallurgy of silver metal is leached with a dilute solution of NaCN in the presence of air (O2)
4Ag + 8CN- +2H2O +O2→ 4[Ag(CN)2] + 4OH -
In this reaction, Ag →Ag+ oxidation number of Ag increases from 0 to +1, hence oxidation
O2→OH- (oxidation number of oxygen decreases from 0 to -2, hence reduction) Hence Leaching of silver is a redox reaction.
2. Magnesite (Magnesium carbonate) is calcined to obtain magnesia, which is used to make refractory bricks. Write the decomposition reaction
Magnesite (Magnesium carbonate) is heated in the absence of oxygen decomposes to form
Magnesium oxide ( Magnesia)
MgCO3→MgO+ CO2  ↑
3. Using Ellingham diagram indicate the lowest temperature at which ZnO can be reduced to Zinc metal by carbon. Write the overall reduction reaction at this temperature
UNIT – 1 METALLURGY5

Ellingham diagram for the formation of ZnO and CO intersects around 1233K Below this temperature, Carbon line lies above Zinc line. Hence ZnO is more stable than CO so the
reduction is thermodynamically not feasible at this temperature range.
However above 1233K carbon line lies below the zinc line, hence carbon can be used as a reducing agent above 1233K.
2Zn +O2→2ZnO ...........1
2C + O2→2CO ..........2
Reversing 1 and adding with equation 2
2ZnO →2Zn+O2
2C + O2→2CO
2ZnO +2C →2Zn + 2CO
 
4. Metallic Sodium is extracted by the electrolysis of brine (aq.NaCl). After electrolysis the electrolytic solution becomes basic in nature. Write the possible electrode
reactions.
Sodium metal is prepared by Down’s process. This involves the electrolysis of fused NaCland CaCl2 at 873K During electrolysis sodium is discharged at the cathode and Cl2 is
obtained at the anode.
NaCl(l)→Na(melt ) + Cl (melt)
Cathode: Na+(melt + e→ Na (s)
Anode: 2Cl− (aq)→ Cl2(g) + 2e
If an aqueous solution of NaCl is electrolysed, H2 is evolved at cathode and Cl2 is evolved at anode. NaOH is obtained in the solution..
UNIT – 1 METALLURGY Reaction5
UNIT – 1 METALLURGY Reaction6
Na + and OH ions to form NaOH .
Hence solution is basic in nature.
 
IV. ADDITIONAL QUESTIONS AND ANSWERS

1. What is concentration of ores?
The removal of non-metallic impurities, rocky materials and siliceous matter (called as gangue) from the ores is known as concentration of ores.
 
2. What is leaching?
In this method crushed ore is allowed to dissolve in a suitable solvent to form a soluble metal salt or complex leaving the gangue undissolved is called leaching.
 
3. What is ammonia leaching?
Crushed ore containing nickel, copper and cobalt is treated with aqueous ammonia under suitable pressure.
Ammonia selectively leaches these metals by forming their soluble complexes namely
[Ni(NH3)6]2+, [Cu(NH3)4]2+ and [Co(NH3)5H2O]3+ from the ore.
The gangue left behind are iron (III) oxides / hydroxides and alumino silicate.
 
4. What is acid leaching?
Sulphide ores ZnS, PbS can be leached with hot aqueous sulphuric acid.
In this process the insoluble sulphide is converted into soluble sulphate and elemental sulphur.
2ZnS(s) +2H2SO4(aq) + O2(g)→2ZnSO4(aq) + 2S(s) + 2H2O
 
5. What are the steps involved in the extraction of crude metal?
1.Conversion of the ore into metal oxide either by roasting or calcination.
2.Reduction of the metal oxide into metal.
 
6. In the extraction of metal, ore is first converted into metal oxide before reduction into metal. Why?
• In the concentrated ore the metal exists in positive oxidation state and hence it is to be reduced to elemental state.
• From the principles of thermodynamics, the reduction of oxide is easier compared to the reduction of other compounds of metal.
• Hence before reduction the ore is first converted into metal oxide.
 
7. Write about the extraction of metal by the process of reduction by hydrogen.
This method can be applied to the oxides of the metals (Fe, Pb, Cu) which are less electropositive than hydrogen.
Ag2O(s) + H2(g)→ Ag(s) + H2O(l)↑
Nickel oxide is reduced to nickel by a mixture of hydrogen and carbon monoxide(water gas)
2NiO(s) + CO(g) + H2(g) → 2Ni(s) + CO2(g) + H2O(l)
 
8. What is auto reduction of metallic ores?
Simple roasting of some of the metallic ores give the crude metal.
Use of reducing agent is not necessary because of low thermal stability (eg) Cinnabar is roasted to give mercury.
HgS(s) + O2(g) → Hg(l) + SO2(g)
 
9. Write the applications of copper.
1. Copper is the first metal used by humans and extended use of its alloy bronze resulted in a new era, ‘Bronze age’.
2.Used for making coins and ornaments along with gold and other metals.
3.Copper and its alloys are used for making wires, water pipes and other electrical parts.
 
10. Write the applications of gold.
1.Gold is one of the expensive and precious metals.
2.Used for coinage and has been used as standard for monetary systems in some countries.
3.Extensively used in jewellery in its alloy form with copper.
4. Used in electroplating to cover other metals with a thin layer of gold, which are used in watches, artificial limb joints, cheap jewellery, dental fillings and electrical connectors.
5.Gold nanoparticles are used for increasing the efficiency of solar cells.
6.Used as a catalyst.
 
11. Write about alumino thermite process.
• In this method a metal oxide such as Cr2O3 is reduced to metal by aluminium.
• Metal oxide (Cr2O3) is mixed with aluminium powder in a fire clay crucible.The reduction process is initiated by ignition mixture of Magnesium power and barium peroxide.
BaO2+ Mg→BaO + MgO
• It is an exothermic process where heat is liberated.
• Temperature = 2400oC Heat liberated = 852kJmol-1.This heat initiate the reduction of Cr2O3 by Al.
UNIT – 1 METALLURGY Reaction7
 
12. What is refining process of a metal?
Metals extracted from its ore contains impurities such as unreacted oxide ore, other metals, non metals etc,. Removal of such impurities from crude metal is known as refining
process of a metal.
 
13. Write about distillation process of refining a metal?
This method is used for low boiling volatile metals like zinc and mercury. In this method impure metal is heated to evaporate and the vapours are condensed to get pure metal.
 
14. Write about liquation process of refining a metal?
• This method is used to remove the impurities with high melting points from metals having relatively low melting points.(eg) Tin, lead, mercury, bismuth.
• The impure metal is placed on sloping hearth of a reverberatory furnace and it is heated just above the melting point of the metal in the absence of air, the molten metal flows
down and impurities are left behind .The molten metal is collected and solidified.
 
15. Give example for the following
1. Frothing agent         2. Collector  3. Depressing agent
Frothing agent            :Pine oil , eucalyptus oil
Collector                     :Sodium ethyl xanthate
Depressing agent       :Sodium cyanide , sodium carbonate
 
16. What is cementation ?
Gold can be recovered by reacting the deoxygenated leached solution with Zinc. In this process Gold is reduced to its elemental state ( zero oxidation state) and the process is
called cementation 
UNIT – 1 METALLURGY Reaction8
 
17. Why Fe, Pb , Cu are reduced by hydrogen ?
The oxides of metal Fe ,Pb , Cu having less electropositive character than hydrogen , these metal oxide can be reduced by hydrogen.
UNIT – 1 METALLURGY Reaction9
 
18. Write about gravity separation or hydraulic wash?
• Ore with high specific gravity is separated from gaugue with low specific gravity by simply washing with running water.
• Finely powdered ore is treated with rapidly flowing current of water.
• Lighter gaugue particles are washed away by the running water.
• This method is used for concentrating native ore such as gold and oxide ores such as haematite(Fe2O3), tin stone(SnO2).
 
19. Write about magnetic separation.
• This method is applicable to ferromagnetic ores.
• It is based on the difference in the magnetic properties of the ore and the impurities.
• Non-magnetic tin stone can be separated from the magnetic impurities wolframite.
• Similarly magnetic ores chromite, pyrolusite can be removed from non magnetic siliceous impurities.
• The crushed ore is poured to an electromagnetic separator with a belt moving over two rollers of which one is magnetic.
• Magnetic part of the ore is attached towards the magnet and falls as a heap close to the magnetic region.
• Non- magnetic part falls away from it.
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20. Write about calcination.
• Calcination is the process in which the concentrated ore is strongly heated in the absence of air.
• During this process water of crystallisation present in the hydrated oxide escapes as moisture.
• Any organic matter present also get expelled leaving the ore porous.
• This method can also be carried out with a limited supply of air.
• During calcination of carbonate ore is decomposed to metal oxide and carbon dioxide is liberated.
UNIT – 1 METALLURGY Reaction10
 
21. Write about Van – Arkel method for refining zirconium/titanium?
• This method is based on the thermal decomposition of gaseous metal compounds to metals.(eg) Titanium and Zirconium.
• Impure titanium is heated in an evacuated vessel with iodine at 550K to form volatiletitanium tetra iodide.
• The impurities do not react with iodine.
UNIT – 1 METALLURGY Reaction11
• Volatile titanium tetraiodide is passed over a tungsten filament at 1800K.
• Titanium tetraiodide is decomposed to pure titanium which is deposited over the filament.Iodine is reused.
UNIT – 1 METALLURGY Reaction12
 
22. Write the applications of aluminium.
1. Used for making heat exchangers/sinks.
2. Used for making our day to day cooking vessels.
3. Used for making aluminium foils for packing, food items.
4. Alloys of aluminium with copper, manganese, magnesium, silicon are light weight and strong hence used in design of aeroplanes and other forms of transport.
5. Due to its high resistance to corrosion, it is used in the design of chemical reactors, medical equipment’s, refrigeration units and gas pipelines.
5. It is a good electrical conductor and cheap, hence used in electrical over head cables with steel core for strength.
 
23. Write the applications of iron.
1.Iron is one the most useful metals and its alloys are used everywhere including bridges, electricity pylons, bicycle chains, cutting tools and rifle barrels.
2.Cast iron is used to make pipes, valves and pump stoves etc.
3.Magnets can be made from iron , its alloys and compounds.
4.Important alloy of iron is stainless steel which is very resistant to corrosion.
5.It is used in architecture, bearings, cutlery, surgical instruments and jewellery.
6.Nickel steel is used for making cables, automobiles, and aeroplane parts.
 
24. Explain froth floatation method.
• This is used to concentrate sulphide ores such as galena (PbS) Zinc blende (ZnS) etc.
• Metallic ore particles preferentially wetted by oil can be separated from gangue.
• Crushed ore is mixed with water and a frothing agent like pine oil or eucalyptus oil.
• A small amount of sodium ethyl xanthate is added as a collector.
• A froth is formed by blowing air through the mixture.
• The collector molecules attach to the ore particles and make them water repellent.
• As a result ore particles wetted by the oil rise to the surface along with the froth.
• The froth is skimmed off and dried to recover the concentrated ore.
• Gangue particles preferentially wetted by water settle at the bottom.
• When sulphide ore contains other metal sulphides as impurities, depressing agents such as sodium cyanide, sodium carbonate etc. are used to selectively prevent other from coming to the froth
• For example , When impurities such as ZnS is present in Galena (PbS) , Sodium cyanide NaCN is added to depresses the flotation property of ZnS) by forming a layer of zinc complex Na2 [Zn(CN)4] on the surface of ZnS.
UNIT – 1 METALLURGY Reaction13
 

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