QuestionIdentify the ONE FALSE statement regarding the electrochemical cell $\mathrm{Co}(\mathrm{~s})\left|\mathrm{CoSO}_{4}(1.00 \mathrm{M}) \| \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}(1.00 \mathrm{M}), \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}(1.00 \mathrm{M})\right| \mathrm{Pt}(\mathrm{~s})$ for which $\mathrm{E}_{\text {cell }}=+1.05 \mathrm{~V}$ . The cell contains a KCl salt bridge. Increasing the concentration of $\mathrm{CoSO}_{4}(\mathrm{aq})$ reduces the cell potential. $\mathrm{K}^{+}$ ions from the salt bridge migrate to the cathode. $\mathrm{Pt}(\mathrm{s})$ is the cathode. $\mathrm{Fe}^{3+}$ ions migrate toward the $\mathrm{Pt}(\mathrm{s})$ electrode. The $\mathrm{Co}^{2+}$ concentration decreases during operation of the cell.

Studdy Solution

STEP 1

1. The electrochemical cell is set up with cobalt and iron half-cells.
2. The cell potential is given as $E_{\text{cell}} = +1.05 \, \text{V}$ .
3. The cell contains a KCl salt bridge.
4. We need to identify the false statement among the given options.

STEP 2

1. Analyze the cell setup and determine the anode and cathode.
2. Evaluate the effect of concentration changes on cell potential.
3. Understand the role of the salt bridge and ion migration.
4. Determine the direction of ion migration during cell operation.
5. Identify the false statement based on electrochemical principles.

STEP 3

Identify the anode and cathode in the cell. The anode is where oxidation occurs, and the cathode is where reduction occurs. In this cell, cobalt is oxidized, and iron is reduced.

STEP 4

Increasing the concentration of $\mathrm{CoSO}_{4}(\mathrm{aq})$ increases the concentration of $\mathrm{Co}^{2+}$ ions, which should increase the cell potential according to the Nernst equation. Therefore, the statement that increasing $\mathrm{CoSO}_{4}$ concentration reduces the cell potential is false.

STEP 5

The KCl salt bridge allows ions to migrate to maintain charge balance. $\mathrm{K}^{+}$ ions migrate to the cathode to balance the charge as $\mathrm{Fe}^{3+}$ is reduced to $\mathrm{Fe}^{2+}$ .

STEP 6

The $\mathrm{Pt}(\mathrm{s})$ electrode is the site of reduction, so it is the cathode. $\mathrm{Fe}^{3+}$ ions migrate toward the $\mathrm{Pt}(\mathrm{s})$ electrode to be reduced.

STEP 7

During the operation of the cell, $\mathrm{Co}^{2+}$ is produced at the anode, so its concentration increases, not decreases. However, this statement is not the false statement we identified in STEP_2.
The false statement is:
"Increasing the concentration of $\mathrm{CoSO}_{4}(\mathrm{aq})$ reduces the cell potential."

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Studdy Solution

STEP 1

1. The electrochemical cell is set up with cobalt and iron half-cells.
2. The cell potential is given as $E_{\text{cell}} = +1.05 \, \text{V}$ .
3. The cell contains a KCl salt bridge.
4. We need to identify the false statement among the given options.

STEP 2

STEP 3

Identify the anode and cathode in the cell. The anode is where oxidation occurs, and the cathode is where reduction occurs. In this cell, cobalt is oxidized, and iron is reduced.

STEP 4

STEP 5

The KCl salt bridge allows ions to migrate to maintain charge balance. $\mathrm{K}^{+}$ ions migrate to the cathode to balance the charge as $\mathrm{Fe}^{3+}$ is reduced to $\mathrm{Fe}^{2+}$ .

STEP 6

The $\mathrm{Pt}(\mathrm{s})$ electrode is the site of reduction, so it is the cathode. $\mathrm{Fe}^{3+}$ ions migrate toward the $\mathrm{Pt}(\mathrm{s})$ electrode to be reduced.

STEP 7

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Studdy Solution

STEP 1

1. The electrochemical cell is set up with cobalt and iron half-cells.2. The cell potential is given as Ecell=+1.05 V E_{\text{cell}} = +1.05 \, \text{V} Ecell​=+1.05V.3. The cell contains a KCl salt bridge.4. We need to identify the false statement among the given options.

STEP 2

STEP 3

Identify the anode and cathode in the cell. The anode is where oxidation occurs, and the cathode is where reduction occurs. In this cell, cobalt is oxidized, and iron is reduced.

STEP 4

STEP 5

The KCl salt bridge allows ions to migrate to maintain charge balance. K+\mathrm{K}^{+}K+ ions migrate to the cathode to balance the charge as Fe3+\mathrm{Fe}^{3+}Fe3+ is reduced to Fe2+\mathrm{Fe}^{2+}Fe2+.

STEP 6

The Pt(s)\mathrm{Pt}(\mathrm{s})Pt(s) electrode is the site of reduction, so it is the cathode. Fe3+\mathrm{Fe}^{3+}Fe3+ ions migrate toward the Pt(s)\mathrm{Pt}(\mathrm{s})Pt(s) electrode to be reduced.

STEP 7

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1. The electrochemical cell is set up with cobalt and iron half-cells.
2. The cell potential is given as $E_{\text{cell}} = +1.05 \, \text{V}$ .
3. The cell contains a KCl salt bridge.
4. We need to identify the false statement among the given options.

The KCl salt bridge allows ions to migrate to maintain charge balance. $\mathrm{K}^{+}$ ions migrate to the cathode to balance the charge as $\mathrm{Fe}^{3+}$ is reduced to $\mathrm{Fe}^{2+}$ .

The $\mathrm{Pt}(\mathrm{s})$ electrode is the site of reduction, so it is the cathode. $\mathrm{Fe}^{3+}$ ions migrate toward the $\mathrm{Pt}(\mathrm{s})$ electrode to be reduced.