1) A Galvanic cell runs on the following reaction:
Co (s) + Cu2+ (aq) → Co2+ (aq) + Cu (s)
Draw a diagram for this Galvanic cell, labeling the electron flow, the anode and cathode, and the positive and negative sides of the Galvanic cell.
2) A Galvanic cell runs on the following reaction:
Al (s) + Fe3+ (aq) → Al3+ (aq) + Fe (s)
Draw a diagram for this Galvanic cell, labeling the electron flow, the anode and cathode, and the positive and negative sides of the Galvanic cell.
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1) Diagram for the Galvanic Cell with the reaction:
Co (s) + Cu2+ (aq) → Co2+ (aq) + Cu (s)
Anode: Co (s) | Co2+ (aq) || Cu2+ (aq) | Cu (s) Cathode
Cathode: The side of the cell where reduction occurs, and redox species accepts electrons.
Anode: The side of the cell where oxidation occurs, and redox species loses electrons.
Electron Flow: From anode to cathode in an external circuit.
Positive side: The side of the cell where cations (positive ions) accumulate. In this case, it is the cathode compartment (Cu2+ (aq) | Cu (s)).
Negative side: The side of the cell where anions (negative ions) accumulate. In this case, it is the anode compartment (Co (s) | Co2+ (aq)).
2) Diagram for the Galvanic Cell with the reaction:
Al (s) + Fe3+ (aq) → Al3+ (aq) + Fe (s)
Anode: Al (s) | Al3+ (aq) || Fe3+ (aq) | Fe (s) Cathode
Cathode: The side of the cell where reduction occurs, and redox species accepts electrons.
Anode: The side of the cell where oxidation occurs, and redox species loses electrons.
Electron Flow: From anode to cathode in an external circuit.
Positive side: The side of the cell where cations (positive ions) accumulate. In this case, it is the cathode compartment (Fe3+ (aq) | Fe (s)).
Negative side: The side of the cell where anions (negative ions) accumulate. In this case, it is the anode compartment (Al (s) | Al3+ (aq)).
To draw the diagram for a Galvanic cell, you will need to understand the basics of the cell and its components. Here's how you can approach each question:
1) A Galvanic cell runs on the following reaction:
Co (s) + Cu2+ (aq) → Co2+ (aq) + Cu (s)
To draw the diagram:
Step 1: Start by drawing a rectangle to represent the Galvanic cell.
Step 2: Label the left side of the rectangle as the anode and the right side as the cathode.
Step 3: Draw vertical lines towards the center of the rectangle to represent the electrodes. Label the left electrode as Co (solid cobalt) and the right electrode as Cu (solid copper).
Step 4: Draw horizontal lines to represent the solutions inside the cell. Label the left side of the vertical line with Cu2+ (aqueous copper ions) and the right side with Co2+ (aqueous cobalt ions).
Step 5: Add a salt bridge (a U-shaped line) connecting the two solutions. Label it as a salt bridge.
Step 6: To indicate electron flow, draw an arrow from the Co electrode to the Cu electrode. This indicates that electrons flow from the anode (cobalt) to the cathode (copper).
2) A Galvanic cell runs on the following reaction:
Al (s) + Fe3+ (aq) → Al3+ (aq) + Fe (s)
To draw the diagram:
Step 1: Start by drawing a rectangle to represent the Galvanic cell.
Step 2: Label the left side of the rectangle as the anode and the right side as the cathode.
Step 3: Draw vertical lines towards the center of the rectangle to represent the electrodes. Label the left electrode as Al (solid aluminum) and the right electrode as Fe (solid iron).
Step 4: Draw horizontal lines to represent the solutions inside the cell. Label the left side of the vertical line with Fe3+ (aqueous iron ions) and the right side with Al3+ (aqueous aluminum ions).
Step 5: Add a salt bridge (a U-shaped line) connecting the two solutions. Label it as a salt bridge.
Step 6: To indicate electron flow, draw an arrow from the Al electrode to the Fe electrode. This indicates that electrons flow from the anode (aluminum) to the cathode (iron).
Remember, in a Galvanic cell, the anode is where oxidation occurs, and electrons flow from the anode to the cathode. The cathode is where reduction occurs. The cell's positive side is where reduction occurs (cathode), and the negative side is where oxidation occurs (anode).