Question

Acetylene torches are used for welding but the thermite reaction can be useful in situations in which acetylene torches are inappropriate. The thermite reaction is Fe2O3 + 2Al yields Al2O3 + 2Fe A welder has 1.873 x 10 to the second power Fe2O3 and 94.51 g Al in his welding kit. How many grams of Aluminum oxide are produced in the reaction? 119.6 g

Answer 1

the mass of aluminum oxide produced in the reaction is 119.6 g.

Step-by-step explanation:

First, we need to determine the limiting reactant in the thermite reaction using stoichiometry. The balanced equation for the reaction is:

Fe2O3 + 2Al → Al2O3 + 2Fe

The molar mass of Fe2O3 is 159.69 g/mol, and the molar mass of Al is 26.98 g/mol.

The number of moles of Fe2O3 in the welder's kit is:

1.873 x 10^2 g Fe2O3 / 159.69 g/mol = 1.174 mol Fe2O3

The number of moles of Al in the welder's kit is:

94.51 g Al / 26.98 g/mol = 3.5 mol Al

According to the balanced equation, the stoichiometric ratio of Fe2O3 to Al is 1:2. Therefore, the number of moles of Al required to react completely with the Fe2O3 is:

1.174 mol Fe2O3 × (2 mol Al / 1 mol Fe2O3) = 2.348 mol Al

Since we only have 3.5 mol Al in the kit, Al is in excess, and Fe2O3 is the limiting reactant.

The theoretical yield of Al2O3 can be calculated based on the number of moles of Fe2O3 in the reaction:

1.174 mol Fe2O3 × (1 mol Al2O3 / 1 mol Fe2O3) × (101.96 g/mol Al2O3) = 119.6 g Al2O3

Therefore, the mass of aluminum oxide produced in the reaction is 119.6 g.