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.
To draw a diagram of the Galvanic cell for the given reaction, follow these steps:
1. Start by drawing a rectangle to represent the Galvanic cell. Label the top side as the positive side and the bottom side as the negative side.
2. Inside the rectangle, draw two compartments separated by a vertical line. Label the left compartment as the anode and the right compartment as the cathode.
3. In the anode compartment, draw a solid line to represent the Co(s) electrode. Label it as Co(s).
4. On the Co(s) electrode, draw an arrow pointing to the right, symbolizing the loss of electrons. Label this arrow as e- (electron flow).
5. In the anode compartment, draw a double vertical line, representing a salt bridge or a porous barrier. Label it accordingly.
6. In the cathode compartment, draw a dashed line to represent the Cu2+ (aq) solution. Label it as Cu2+ (aq).
7. In the Cu2+ (aq) solution, draw a solid line to represent the Cu(s) electrode. Label it as Cu(s).
8. On the Cu(s) electrode, draw an arrow pointing to the left, symbolizing the gain of electrons. Label this arrow as e- (electron flow).
9. Finally, label the anode and cathode compartments accordingly.
The final diagram should look like this:
_______________________________________
| |
| Anode |
| Co(s) | Co2+ (aq) |
| __________________||______________ |
| | | |
| | Salt Bridge / | |
| | Porous Barrier | |
| | | |
| |__________________________________| |
| |
| Cathode |
| Cu2+ (aq) | Cu(s) |
|_______________________________________|
Remember that the electrons flow from the anode to the cathode (left to right in this case). The anode is where the oxidation half-reaction occurs (Co(s) → Co2+ (aq) + 2e-) and the cathode is where the reduction half-reaction occurs (Cu2+ (aq) + 2e- → Cu(s)).
To draw a diagram for this Galvanic cell, follow these steps:
1. Identify the half-reactions: In this case, we have the following two half-reactions:
- Co (s) → Co2+ (aq) + 2e- (oxidation half-reaction)
- Cu2+ (aq) + 2e- → Cu (s) (reduction half-reaction)
2. Identify the anode and cathode: The anode is where oxidation occurs, and the cathode is where reduction occurs. In this case, Co (s) undergoes oxidation to Co2+ at the anode, and Cu2+ undergoes reduction to Cu (s) at the cathode.
3. Label the electron flow: Since oxidation involves the loss of electrons and reduction involves the gain of electrons, the electrons flow from the anode to the cathode. Therefore, you can label the electron flow from left to right in the diagram.
4. Label the positive and negative sides: The positive side of the Galvanic cell is where the reduction half-reaction occurs (cathode), and the negative side is where the oxidation half-reaction occurs (anode). Hence, label the positive and negative sides accordingly.
Here is a diagram of the Galvanic cell:
Co (s) Co2+ (aq) || Cu2+ (aq) Cu (s)
(anode) (cathode)
negative positive
side side
Electrons flow: ---->
Please note that the vertical lines "||" represent a salt bridge or a porous barrier that allows ion flow to maintain charge balance between the half-cells.