Answer:
54 g of Aluminium were oxidized
Explanation:
The equation for the reaction:
4Al(s)+3O₂(g)→2Al₂O₃(s)
We are required to calculate the mass of Aluminium that reacted;
Step 1: Calculating the number of moles Aluminum oxide
Mass of Aluminium oxide = 102 g
Molar mass of Al₂O₃ = 101.96 g/mol
Number of moles = Mass ÷ Molar mass
= 102 g ÷ 101.96 g/mol
= 1 mole
Step 2: Number of moles of Aluminium oxidized
From the equation, the mole ratio of Al to Al₂O₃ is 4 : 2
Therefore; Moles of Al is (4/2)(1) is 2 moles
2 moles of Aluminium were oxidized
Step 3: Mass of Aluminium oxidized
Mass = Number of moles × Molar mass
Molar mass of Aluminium is 27 g/mol
Therefore;
Mass of Aluminium = 2 moles × 27 g/mol
= 54 g
Therefore, 54 g of Aluminium were oxidized
