\( \mathrm{Fe}_{2} \mathrm{O}_{3}+\mathrm{Al} \longrightarrow \mathrm{Al}_{2} \mathrm{O}_{3}+\mathrm{Fe}+\mathrm{Heat} \) Balance the above reaction

To balance the reaction \( \mathrm{Fe}_{2} \mathrm{O}_{3} + \mathrm{Al} \longrightarrow \mathrm{Al}_{2} \mathrm{O}_{3} + \mathrm{Fe} + \mathrm{Heat} \), we start by ensuring that the number of each type of atom is the same on both sides. The balanced equation is: \[ 2 \mathrm{Fe}_{2} \mathrm{O}_{3} + 6 \mathrm{Al} \longrightarrow 3 \mathrm{Al}_{2} \mathrm{O}_{3} + 4 \mathrm{Fe} \] This means we have 2 iron (III) oxide molecules reacting with 6 aluminum atoms to produce 3 aluminum oxide molecules and 4 iron atoms. The adjustment of coefficients ensures that the law of conservation of mass is upheld without changing the actual substances involved!