The mass of carbon anode consumed (giving of carbon dioxide) in the production of $270 k g$ aluminium metal bum bauxite by Hall process is: (Atomic mass $A l = 27$ )

180

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270

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540

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90

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Solution

The correct option is D $90$ kg
The chemical reaction for the Hall process is given by
$2 A l_{2} O_{3} + 3 C \to 4 A l + 3 C O_{2}$
Moles of aluminium produced $= \frac{270000}{27} = 10000$
According to the reaction,
$10000 k g$ moles of aluminium can be produced by consuming $2500 \times 3 = 7500 m o l e s$ of Carbon
Hence mass of carbon= $12 \times 7500 = 90000 g = 90 k g$

Therefore, D is the correct answer

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Similar questions

Q. The mass of carbon anode consumed (giving the only carbon dioxide) in the production of

270 k g

of aluminium metal from bauxite by the Hall process is:
[Atomic mass :

A l = 27

]

Q. the mass of carbon anode consumed (giving only carbon dioxide) in the production of

270 K g

of aluminium metal from bauxite by the Hall's process is:

2 A l_{2} O_{3} + 3 C \to 4 A l + 3 C O_{2}

Q. Aluminium oxide may be electrolysed at

1000^{\circ} C

to furnish aluminium metal (Atomic mass

= 27 a m u; 1 f a r a d a y = 96500 c o u l o m b

). The cathode reaction is:

A l^{3 +} + 3 e^{-} \to A l

To prepare

5.12 k g

of aluminium metal by this method we would require.

Aluminium oxide may be electrolyte at 1000 $^{0}$ C to furnish aluminium metal (Atomic mass = 27 amu, 1 Faraday = 96,500 Coulombs). The cathode reaction is $A l^{3} + 3 e^{-} \to A l^{o}$ . To prepare 5.12 kg of aluminium metal by this method would require:

Q. 2.4 kg of carbon is made to react with 1.35 kg of aluminium to form

A l_{4} C_{3} .

The maximum amount of aluminium carbide formed is:

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The mass of carbon anode consumed (giving of carbon dioxide) in the production of 270 kg aluminium metal bum bauxite by Hall process is: (Atomic mass Al=27)

The mass of carbon anode consumed (giving of carbon dioxide) in the production of $270 k g$ aluminium metal bum bauxite by Hall process is: (Atomic mass $A l = 27$ )