| (I) Heating impure metal CO and distilling the resulting volatile carbonyl \[\left( b.p.\text{ }43{}^\circ C \right)\] and finally decomposition at \[150{}^\circ -200{}^\circ C\] to get the pure metal |
| (II) Heating the sulphide ore in air until a part is converted to oxide and then furher heating in the absence of air to let the oxide react with unchanged metal sulphide |
| (III) Electrolysis of the molten electrolyte containing approximately equal amounts of the metal chloride and \[NaCl\] to obtained the metal |
| The processes used for obtaning magnesium, nickel and copper are respectively: |
A) (I), (II) and (III)
B) (II), (III) and (I)
C) (III), (I) and (II)
D) (II), (I) and (III)
Correct Answer: C
Solution :
[c] (I) \[\underset{(impure)}{\mathop{Ni}}\,+4CO\xrightarrow{50{}^\circ C}\underset{(volite)}{\mathop{\left[ Ni{{\left( CO \right)}_{4}} \right]}}\,\] \[\xrightarrow{230{}^\circ C}\underset{(pure)}{\mathop{Ni}}\,+4CO\uparrow \] (II) \[C{{u}_{2}}S+\frac{3}{2}{{O}_{2}}\xrightarrow{\Delta }C{{u}_{2}}O+S{{O}_{2}}\] \[C{{u}_{2}}S+2C{{u}_{2}}O\xrightarrow[temp.]{high}6Cu+S{{O}_{2}}\] (III) \[MgC{{l}_{2}}(g)\xrightarrow{electrolysis}M{{g}^{2+}}(l)+2C{{l}^{-}}(l)\] At cathode: \[M{{g}^{2+}}+2{{e}^{-}}\xrightarrow{{}}Mg(s)\] At anode: \[2C{{l}^{-}}\left( l \right)\xrightarrow{{}}C{{l}_{2}}\left( g \right)+2{{e}^{-}}\]
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