3Fe2+(aq) + 2Al(s) --> 3Fe(s) + 2Al3+(aq)
Which of the following statements is true about Fe2+?
1.Fe2+ is losing electrons.
2.Fe2+ is oxidized.
3.Fe2+ is the oxidizing agent.
4.Fe2+ is the reducing agent.
Well, it seems like Fe2+ is in the spotlight here! Fe2+ is indeed losing electrons (statement 1), so it must be oxidized (statement 2). However, it can't be both the oxidizing agent and the reducing agent. That would be like trying to juggle bananas and catch them at the same time! So, we can rule out statements 3 and 4.
To determine the true statement about Fe2+ in the given chemical reaction, we need to understand the concept of oxidation and reduction.
Oxidation is the process in which an atom or ion loses electrons, while reduction is the process in which an atom or ion gains electrons. The substance that loses electrons is called the reducing agent, while the substance that gains electrons is called the oxidizing agent.
In the given reaction: 3Fe2+(aq) + 2Al(s) → 3Fe(s) + 2Al3+(aq)
Fe2+ is transformed into Fe(s), meaning it is gaining electrons and being reduced.
Therefore, the true statement about Fe2+ in the reaction is:
4. Fe2+ is the reducing agent.
To determine which of the statements is true about Fe2+ in the given reaction, we need to understand the concepts of oxidation and reduction.
Oxidation is the process in which a substance loses electrons, while reduction is the process in which a substance gains electrons. In a redox reaction, there is always an oxidation reaction and a reduction reaction occurring simultaneously.
Looking at the given reaction:
3Fe2+(aq) + 2Al(s) --> 3Fe(s) + 2Al3+(aq)
We see that Fe2+(aq) is being converted to Fe(s). This means that Fe2+ is gaining electrons (from 2+ to 0 charge), which indicates a reduction process. Therefore, Fe2+ is being reduced.
So, the correct statement is:
4. Fe2+ is the reducing agent.
To determine the oxidizing agent, we look at the other species involved in the reaction. In this case, Al(s) is being converted to Al3+(aq), which means it is losing electrons (from 0 to 3+ charge), indicating an oxidation process. Therefore, Al is being oxidized.
So, the correct statement about Al in this reaction is:
2. Fe2+ is oxidized.
In the given reaction, Fe2+ is not the overall oxidizing agent or reducing agent. The reducing agent is the species that gets oxidized, which is Al in this case. The oxidizing agent is the species that gets reduced, which is Fe2+ in this case.
So, the correct statement is:
4. Fe2+ is the reducing agent.
it gains electrons.
Al loses electrons, it is oxidized, something oxidizing agent gains those electrons.