A student constructs a galvanic cell that has a strip of iron metal immersed in a solution of

0.1M Fe(NO3)2 as one half-cell and a strip of zinc metal immersed in a solution of 0.1M Zn(NO3)2
as the other half-cell. The measured cell potential is less than zero when the positive terminal of
the voltmeter is attached to the zinc strip and the negative terminal is attached to the iron strip.

Which half-cell is the anode (Fe or Zn)?

Which half-cell is the cathode?

Do the electrons flow from Zn to Fe or vice versa?

Which metal is more “active” Zn or Fe?

The electrode reactions are

Zn ==> Zn^2+ + 2e
Fe^2+ + 2e ==> Fe
The anode is where oxidation occurs; therefore, Zn is the anode and it is the negative electrode. Electrons flow from Zn to Fe. Zn is more "active" than Fe.

To determine the answers to these questions, we need to analyze the given information about the galvanic cell. The first step is to understand the concepts of anode, cathode, and cell potential.

In a galvanic cell, the anode is the electrode where oxidation occurs, and electrons are lost. The cathode is the electrode where reduction occurs, and electrons are gained. The flow of electrons goes from the anode to the cathode. The cell potential is a measure of the tendency for the reaction to occur, and a negative cell potential indicates a non-spontaneous reaction.

Now, let's analyze the information given. We have two half-cells:

1. A strip of iron metal immersed in a solution of 0.1M Fe(NO3)2
2. A strip of zinc metal immersed in a solution of 0.1M Zn(NO3)2

Given that the measured cell potential is less than zero when the positive terminal of the voltmeter is connected to the zinc strip and the negative terminal is connected to the iron strip, we can make the following determinations:

1. The anode: The strip where oxidation occurs is the anode. Since the potential is negative when the zinc strip is connected to the positive terminal, the zinc strip is the anode.

2. The cathode: The strip where reduction occurs is the cathode. Since the potential is negative when the zinc strip is connected to the positive terminal, the iron strip is the cathode.

3. The flow of electrons: Electrons flow from the anode to the cathode. In this case, they will flow from the zinc strip to the iron strip.

4. The more "active" metal: The metal that acts as the anode (where oxidation occurs) is considered to be more active. In this case, zinc is the anode, indicating that it is more active than iron.

To summarize:
- The anode is the zinc strip.
- The cathode is the iron strip.
- Electrons flow from Zn to Fe.
- Zinc is more "active" than iron.

Remember, when analyzing galvanic cells, it is essential to compare the reactions happening at each electrode and consider the measured cell potential to determine the anode, cathode, flow of electrons, and the relative activity of metals.

To determine which half-cell is the anode and which is the cathode, and to determine the direction of electron flow and the metal that is more "active" between zinc (Zn) and iron (Fe), we can use the information provided about the measured cell potential.

Given that the measured cell potential is less than zero when the positive terminal of the voltmeter is attached to the zinc strip and the negative terminal is attached to the iron strip, we can conclude the following:

1. The anode is the half-cell where oxidation occurs. In this case, zinc (Zn) is oxidized to Zn2+ ions, which implies that the half-cell with the zinc metal strip is the anode.

2. The cathode is the half-cell where reduction occurs. In this case, iron (Fe2+) ions from the Fe(NO3)2 solution are reduced to iron metal. Therefore, the half-cell with the iron strip is the cathode.

3. Electrons flow from the anode to the cathode, which means they flow from the zinc strip to the iron strip.

4. The metal that is more "active" is the one that tends to lose electrons more easily, which signifies a stronger reducing agent. In this case, since zinc (Zn) is being oxidized (loses electrons) at the anode, it is more "active" than iron (Fe).

To summarize:
- The anode is the half-cell with the strip of zinc metal (Zn).
- The cathode is the half-cell with the strip of iron metal (Fe).
- Electrons flow from the zinc (Zn) strip to the iron (Fe) strip.
- Zinc (Zn) is more "active" than iron (Fe).