Balance the equation: Al + Fe2O3 → Al2O3 + Fe.

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Multiple Choice

Balance the equation: Al + Fe2O3 → Al2O3 + Fe.

Explanation:
Balancing this redox reaction comes from matching both atoms and electrons between the sides. Aluminum starts at oxidation state 0 and ends up as Al2O3 where aluminum is +3. That means each aluminum atom loses 3 electrons. In Fe2O3, iron is +3, so each iron atom would gain electrons to become Fe(0). Fe2O3 has two Fe atoms, so it accepts 6 electrons in total. That requires two aluminum atoms to supply those 6 electrons (2 × 3 = 6). Oxygen balance also guides the coefficients: Fe2O3 contains 3 oxygen atoms, and Al2O3 contains 3 oxygen atoms, so one Fe2O3 can produce one Al2O3 without changing the oxygen count. Putting it together gives: 2 Al + Fe2O3 → Al2O3 + 2 Fe. This satisfies the balance for Al, Fe, and O, and also reflects the electron transfer in this redox process. Other attempted multiples would misbalance either aluminum, iron, or oxygen atoms.

Balancing this redox reaction comes from matching both atoms and electrons between the sides. Aluminum starts at oxidation state 0 and ends up as Al2O3 where aluminum is +3. That means each aluminum atom loses 3 electrons. In Fe2O3, iron is +3, so each iron atom would gain electrons to become Fe(0). Fe2O3 has two Fe atoms, so it accepts 6 electrons in total. That requires two aluminum atoms to supply those 6 electrons (2 × 3 = 6).

Oxygen balance also guides the coefficients: Fe2O3 contains 3 oxygen atoms, and Al2O3 contains 3 oxygen atoms, so one Fe2O3 can produce one Al2O3 without changing the oxygen count.

Putting it together gives: 2 Al + Fe2O3 → Al2O3 + 2 Fe. This satisfies the balance for Al, Fe, and O, and also reflects the electron transfer in this redox process. Other attempted multiples would misbalance either aluminum, iron, or oxygen atoms.

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