If you put a piece of iron in an aqueous solution of blue Cu2+ ions the spontaneous redox reaction

Fe+ Cu2+„³ Fe2+ Cu
Will occur. An aqueous solution of Fe2+ ions is red-brown
a. What is oxidized
b. What is reduced
c. What is the oxidizing agent
d. What is the reducing agent
e. What will happen to the piece of iron over time
f. Do the electrons move from the oxidizing agent to the reducing agent or vice versa.
g. How could you use this reaction to make a battery? Explain and show your battery using a nail and a penny has your source of iron and copper

See your last post.

a. In the given reaction, iron (Fe) is oxidized.

To identify the species being oxidized, we need to compare the oxidation states of the elements before and after the reaction. In this case, the iron (Fe) goes from a neutral state (0) to a +2 oxidation state, indicating that it has lost electrons. This loss of electrons is characteristic of oxidation.

b. Copper ions (Cu2+) are reduced.

Again, comparing the oxidation states, we see that copper (Cu) goes from a +2 oxidation state to a neutral state (0), indicating that it has gained electrons. This gain of electrons is characteristic of reduction.

c. The oxidizing agent is the species that causes oxidation, in this case, Cu2+ ions.

The oxidizing agent accepts electrons from the species being oxidized (Fe). Cu2+ ions are reduced to Cu during the reaction, so they act as the oxidizing agent.

d. The reducing agent is the species that causes reduction, in this case, Fe.

The reducing agent donates electrons to the species being reduced (Cu2+ ions). Fe is oxidized to Fe2+ during the reaction, so it acts as the reducing agent.

e. Over time, the piece of iron will undergo corrosion.

In the reaction, iron undergoes oxidation, meaning it loses electrons. As a result, the iron ions (Fe2+) formed can react with water and oxygen present in the atmosphere to form iron oxide (rust). This leads to the gradual degradation of the iron over time.

f. In a spontaneous redox reaction, electrons move from the reducing agent to the oxidizing agent.

The reducing agent (Fe) donates electrons to the oxidizing agent (Cu2+), causing reduction and oxidation to occur simultaneously. In this case, Fe loses electrons, while Cu2+ gains electrons.

g. You can use this reaction to make a simple battery by constructing a galvanic (voltaic) cell.

To make a battery, you would need two different metals, each in contact with a different aqueous solution containing their respective ions. In this case, a nail (source of iron) can act as the anode (the negative electrode) and a penny (made of copper) can act as the cathode (the positive electrode).

The nail is placed in an aqueous solution containing Fe2+ ions, while the penny is placed in an aqueous solution containing Cu2+ ions. These two solutions should be connected using a salt bridge or some other appropriate conductor to facilitate ion flow.

As the iron nail gets oxidized and loses electrons, they travel through an external circuit from the anode (nail) to the cathode (penny). This movement of electrons can be used to power an electrical device connected to the circuit. Meanwhile, copper ions in the solution are reduced at the penny electrode, completing the redox reaction. This flow of electrons generates a potential difference or voltage, creating a battery-like setup.