Final answer:
In the thermite reaction, aluminium is oxidized and acts as the reducing agent, while iron oxide is reduced to form iron. Statement E is incorrect, as three electrons are not transferred from each Al atom to each Fe atom; instead, the transfer involves a total of 9 electrons from 3 Al atoms to 2 Fe3+ ions.
Step-by-step explanation:
The thermite reaction involves aluminium being oxidized and iron being reduced. The correct balanced chemical equation for the thermite reaction is:
2 Al(s) + Fe₂O₃(s) → 2 Fe(s) + Al₂O₃(s) +heat
This reaction is highly exothermic, producing enough heat to melt the iron. Based on the student's provided equation (which follows a multiple of the correct stoichiometry), we can analyze each statement:
- A. Aluminium is oxidized: true, as Al goes from 0 to +3 in oxidation state.
- B. Iron is reduced: true, as Fe3O4 is reduced to Fe.
- C. Oxidation number of Al goes from 0 to +3: true, evident from the aluminum gaining an oxidation state of +3.
- D. Aluminium is the reducing agent: true, since it loses electrons and reduces Fe3O4.
- E. Three electrons are transferred from each Al atom to each Fe atom: this statement is not true. In reality, 3 Al atoms donate a total of 9 electrons to 2 Fe3+ ions to reduce them to Fe. Thus, it's not a one-to-one transfer of electrons from each Al to each Fe.
The incorrect statement is E: Three electrons are transferred from each Al atom to each Fe atom.