Question

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

• A. 180 kg
• B. 120 kg
• C. 360 kg
• D. 90 kg

Answer 1

The Correct Option is D

 To determine the mass of carbon anode consumed in the production of 270 kg of aluminum metal using the Hall process, we need to understand the chemical reactions involved in this process and use stoichiometry to calculate the required amount of carbon.

Firstly, the Hall process is an electrolytic process used to extract aluminum from aluminum oxide (Al₂O₃). The overall reaction involved in this process can be represented as follows:

\(2 \text{Al}_2\text{O}_3 + 3\text{C} \rightarrow 4\text{Al} + 3\text{CO}_2\)

This equation tells us that 2 moles of aluminum oxide react with 3 moles of carbon to produce 4 moles of aluminum and 3 moles of carbon dioxide (CO₂).

1. First, calculate the moles of aluminum produced:
   • The molar mass of aluminum (Al) is 27 g/mol.
   • Given that we have 270 kg of aluminum, the number of moles of aluminum is calculated as follows:
2. According to the balanced equation, 4 moles of Al are produced from 3 moles of carbon. Thus, moles of carbon required is calculated by:
3. Finally, calculate the mass of carbon consumed:
   • The molar mass of carbon (C) is 12 g/mol.
   • The mass of carbon consumed is:

Therefore, the mass of carbon anode consumed in the production of 270 kg of aluminum is 90 kg.