Which of the following statements are true for the reaction of Fe2O3 with aluminium? 1. It is known as the 'thermite reaction'. 2. The heat evolved is used for welding purpose. 3. Aluminium metal acts as an oxidizing agent. 4. Molten Fe and Al are formed at the end of the reaction. Select the correct answer using the code given below.

The reaction between iron(III) oxide (Fe2O3) and aluminium is a highly exothermic displacement reaction known as the 'thermite reaction' [1]. The heat generated is so intense (reaching temperatures above 2500°C) that the iron produced is in a molten state, which is utilized for welding railway tracks and cracked machine parts [2]. In this redox process, aluminium acts as a reducing agent because it has a stronger affinity for oxygen than iron, while Fe2O3 acts as the oxidizing agent. The products of the reaction are molten iron (Fe) and solid or slag aluminium oxide (Al2O3); aluminium itself is consumed as a reactant and does not remain as a molten metal product. Therefore, statements 1 and 2 are correct, while statement 3 is false (Al is a reducing agent) and statement 4 is false (only Fe is molten; Al2O3 is the other product).

Sources

1. [1] Science , class X (NCERT 2025 ed.) > Chapter 3: Metals and Non-metals > 3MnO2 (s) + 4Al(s) → 3Mn(l) + 2Al2O3 (s) + Heat > p. 52
2. [2] https://www.osti.gov/servlets/purl/1491647