Al + Fe^3+ -> Al^3+ + Fe^2+
which substance is being oxidized?which is being reduced?
which substance is oxidizing agent? reducing agent?
how many electrons are exchanged in the reaction above?
also: why is Fe^3+ not reduced to Fe?
Oxidation is the loss of electrons.
Reduction is the tgain of electrons.
The substance being oxidized is the reducing agent.
The substance being reduced is the oxidizing agent.
Al goes from an oxidation state of 0 on the left to +3 on the right. Therefore, it lost three electrons and is oxidized.
Fe^+3 goes from an oxidation state of +3 on the left to +2 on the right; therefore, it gained one electron and is reduced.
To determine the oxidizing agent and reducing agent, you need to consider the change in oxidation states of each element.
In this reaction, aluminum (Al) is going from an oxidation state of 0 to +3. This means that it is losing three electrons and being oxidized. Therefore, Al is the substance being oxidized and the reducing agent.
On the other hand, iron (Fe) is going from an oxidation state of +3 to +2. This means that it is gaining one electron and being reduced. Therefore, Fe is the substance being reduced and the oxidizing agent.
In terms of the number of electrons exchanged, Al loses three electrons and Fe gains one electron, so a total of four electrons are exchanged in the reaction.
Now, addressing why Fe^3+ is not reduced directly to Fe. The reaction you provided is a simplified representation of a redox reaction. In reality, the reaction likely involves additional steps, such as the transfer of electrons through a solid conductor or the involvement of other species in a complex reaction mechanism. The Fe^3+ ion may not be directly reduced to Fe because of such considerations.