1. Write the Balanced Chemical Equation:

The thermite reaction is:

Fe₂O₃ (s) + 2 Al (s) → 2 Fe (l) + Al₂O₃ (s)

2. Calculate Moles of Reactants:

* Moles of Fe₂O₃:

- Molar mass of Fe₂O₃ = 159.69 g/mol

- Moles = (8.368 g) / (159.69 g/mol) = 0.0524 mol

* Moles of Al:

- Molar mass of Al = 26.98 g/mol

- Moles = (9.825 g) / (26.98 g/mol) = 0.364 mol

3. Determine the Limiting Reactant:

- From the balanced equation, 1 mole of Fe₂O₃ reacts with 2 moles of Al.

- The mole ratio of Fe₂O₃ to Al is 1:2.

- For the given amount of Fe₂O₃ (0.0524 mol), we would need 0.0524 mol * 2 = 0.1048 mol of Al.

- We have more Al (0.364 mol) than we need. Therefore, Fe₂O₃ is the limiting reactant.

4. Calculate Moles of Excess Reactant (Al) Consumed:

- Since Fe₂O₃ is the limiting reactant, it determines how much Al reacts.

- From the balanced equation, 1 mole of Fe₂O₃ reacts with 2 moles of Al.

- So, 0.0524 mol of Fe₂O₃ will react with 0.0524 mol * 2 = 0.1048 mol of Al.

5. Calculate Moles of Excess Reactant (Al) Remaining:

- Initial moles of Al - moles of Al consumed = moles of Al remaining

- 0.364 mol - 0.1048 mol = 0.2592 mol

Answer: There are 0.2592 moles of aluminum remaining after the reaction.