Question

The mass of carbon anode consumed (giving only
carbondioxide) in the production of 270 kg of aluminium
metal from bauxite by the Hall process is (Atomic mass:
Al = 27)
(a) 270 kg (b) 540 kg (c) 90 kg (d) 180 kg

Answer 1

90kg of carbon is utilized.

Explanation:

• Hall - Heroult process is the process of aluminium refining.

• This process utilizes carbon anode which gives electrons and gets oxidised to form carbon dioxide.

• This electron is given to aluminium which is reduced from aluminium oxide to metallic aluminum.

• The reaction involved is

• 2Al2O3 + 3C = 4 Al + 3CO2.

• So, for every 4 moles of aluminium produced, 3 moles of carbon is utilized.

• So, for, 10,000 moles of aluminium produced, $\frac{10000 \times4}3$ = 7500 moles of carbon is utilized.

• So, weight of carbon utilized = $7500 \times 12$gram = 90000gram = 90kg.

For more information about Hall Process,

https://brainly.in/question/6070847

Explain hall heroult process - Brainly.in

https://brainly.in/question/9628010

Difference between Hall's process and hoops process - Brainly.in

Answer 2

The mass of carbon anode consumed to give carbondioxide is 90 kg

Explanation:

In Hall process, Aluminium is extraction includes the following chemical reactions

$2 A l_{2} O_{3} \longrightarrow 4 A l+3 O_{2}$

$4 C+3 O_{2} \longrightarrow 2 C O_{2}+2 C O \uparrow$

For consuming of carbondioxide, the reaction possible is

$2 \mathrm{Al}_{2} \mathrm{O}_{3}+3C_{3 \times 12=36} \longrightarrow \underset{4 \times 27=108}{4 \mathrm{Al}}+3 \mathrm{CO}_{2}$

From the above equation, we can observe that,

For obtaining 108 kg of Aluminium 36 kg of Carbon is required

Therefore to get 270 kg of Aluminium the required carbon is

$=\frac{36}{108} \times 270=90 k g$

Therefore, the correct answer is option (c)