Practicing Success
In a thermite process, the reducing agent is |
C Zn Na Al |
Al |
The correct answer is option 4. Al. The thermite process is a highly exothermic reaction in which a metal oxide is reduced by a more reactive metal to produce molten metal and an oxide slag. The most common thermite reaction involves the reduction of iron(III) oxide (\(Fe_2O_3\)) by aluminum (\(Al\)) to produce iron and aluminum oxide (\(Al_2O_3\)). The chemical equation for the thermite reaction involving iron(III) oxide and aluminum is: \(Fe_2O_3(s) + 2Al(s) \rightarrow 2Fe(l) + Al_2O_3(s) \) In this reaction:
Now, let us delve into the role of aluminum as the reducing agent in the thermite process: 1. Reducing Agent: A reducing agent is a substance that donates electrons to another substance (the oxidizing agent) during a chemical reaction. In the thermite reaction, aluminum serves as the reducing agent. When aluminum reacts with iron(III) oxide, it donates electrons to reduce iron(III) ions to iron metal: \[ 2Al(s) \rightarrow 2Al^{3+}(aq) + 6e^- \] \[ Fe_2O_3(s) + 6e^- \rightarrow 2Fe(l) + 3O^{2-}(aq) \] \[ 2Al(s) \rightarrow 2Al^{3+}(aq) + 6e^- \] 3. Reduction of Iron(III) Oxide: Iron(III) oxide gains electrons from aluminum, resulting in the reduction of iron(III) ions to iron metal: \[ Fe_2O_3(s) + 6e^- \rightarrow 2Fe(l) + 3O^{2-}(aq) \] \[ Fe_2O_3(s) + 2Al(s) \rightarrow 2Fe(l) + Al_2O_3(s) \] In summary, aluminum serves as the reducing agent in the thermite process, donating electrons to reduce iron(III) oxide to iron metal while undergoing oxidation itself. This reaction releases a significant amount of heat energy and is used for various industrial and military applications. |