How Much Aluminum Can Be Derived from 1020g of Aluminum Oxide?
Understanding the process of producing aluminum from aluminum oxide is crucial for industries that rely heavily on this metal. This article will guide you through the steps to calculate how much aluminum can be formed from 1020 grams of aluminum oxide (Al2O3) using basic principles of chemical stoichiometry and the properties of aluminum oxide. This topic is highly relevant for students, chemists, and engineers involved in material science and industrial processes.
Stoichiometric Calculation of Aluminum from Aluminum Oxide
To determine the mass of aluminum that can be derived from 1020 grams of aluminum oxide, we need to use stoichiometry based on the balanced chemical reaction for the reduction of aluminum oxide to aluminum. The balanced equation for this reaction is:
2 Al2O3 → 4 Al 3 O2
Step-by-Step Calculation Process
1. Calculate the Molar Mass of Aluminum Oxide (Al2O3)
The molar mass of a compound is the sum of the atomic masses of all atoms in the molecule. For aluminum oxide (Al2O3), the atomic masses are known as:
- Aluminum (Al): 26.98 g/mol - Oxygen (O): 16.00 g/mol
The molar mass of Al2O3 can be calculated as:
Molar mass of Al2O3 2 × 26.98 g/mol 3 × 16.00 g/mol 53.96 g/mol 48.00 g/mol 101.96 g/mol
2. Determine the Number of Moles of Aluminum Oxide (Al2O3) in 1020 grams
The number of moles of a substance is given by the formula:
n mass / molar mass
Using the molar mass calculated, we can find the number of moles of aluminum oxide:
nAl2O3 1020 g / 101.96 g/mol ≈ 10.00 mol
3. Use Stoichiometry to Find the Moles of Aluminum (Al) Produced
According to the balanced chemical equation, 2 moles of Al2O3 produce 4 moles of Al. Therefore, 1 mole of Al2O3 will produce 2 moles of Al. We can use this stoichiometric relationship to find the moles of Al produced:
Moles of Al 10.00 mol Al2O3 × (4 mol Al / 2 mol Al2O3) 20.00 mol Al
4. Calculate the Mass of Aluminum Produced
The mass of a substance is the product of the number of moles and the molar mass. For aluminum, the molar mass is 26.98 g/mol. Therefore, the mass of aluminum produced can be calculated as:
Mass of Al moles of Al × molar mass of Al 20.00 mol × 26.98 g/mol 539.6 g
Conclusion
In conclusion, the mass of aluminum that can be derived from 1020 grams of aluminum oxide (Al2O3) is approximately 539.6 grams. This process is a fundamental calculation in the production of aluminum and serves as a basic example of how stoichiometry is applied in chemical reactions and material science.
Key Takeaways
Understanding the properties of aluminum oxide and its molar mass. Applying stoichiometric principles to relate the masses of different reactants and products. Calculating the amount of a desired product from the given amount of reactant.Frequently Asked Questions (FAQ)
What is the molar mass of aluminum oxide?The molar mass of aluminum oxide (Al2O3) is 102 g/mol, calculated as 2 × 26.98 (Al) 3 × 16.00 (O) 102 g/mol.
How does the stoichiometry of the reaction between aluminum oxide and aluminum differ?The balanced equation for the reaction between aluminum oxide and aluminum is 2 Al2O3 → 4 Al 3 O2. This indicates that 2 moles of aluminum oxide produce 4 moles of aluminum, and 1 mole of aluminum oxide produces 2 moles of aluminum.
Can the mass of aluminum be precisely calculated from the given mass of aluminum oxide?Yes, the mass of aluminum can be precisely calculated using stoichiometry, provided the correct molar masses and the balanced chemical equation.