Cu (s) →Cu2+ (aq) + 2e-
Zn (s) →Zn2- (aq) + 2e-
Independent Variable: Temperature of the electrolytes (°C)
Dependant Variable: Voltage (V)
Controlled Variables:
-
Nature of electrodes: The electrodes will be of the same elements i.e. Copper and Zinc. Changing the nature of the electrodes will change the voltage since different elements produce different forms of ions which then affects the voltage of the cell.
-
Size of electrodes: The size of electrodes will be kept constant to 6cm x 1cm. Increasing the size of electrodes means that the electrodes will react produce more ions hence increasing the voltage of the cell.
-
Nature of ion transfer: A salt bridge (dipped in KNO3) will be used as a pathway for the ion transfer between the two half cells. Changing the nature of ion transfer will change the amount of ions are transferred between the half cells hence affecting the voltage.
-
The concentration of the electrolytes: is kept constant. A constant amount of metal salt will be added to make each electrolyte. Having a varying concentration will affect the amount of ions produced hence varying the voltage accordingly.
-
Voltmeter: The voltmeter is kept constant since changing the voltmeter can affect the voltage since different voltmeters may have different resistance which may affect the readings.
Materials required
- Copper strip, 6cm x 1cm
- Zinc strip, 6cm x 1cm
-
CuSO4 solution, 0.99M ± 0.01M
-
ZnSO4 solution, 0.99M ± 0.01M
-
KNO3 solution, 1.99M ± 0.01M
- Distilled water, 300mL ± 1mL
- Beakers (3), 250mL ± 50mL
- Graduated cylinder (100mL ± 1mL)
- Digital Voltmeter with crocodile wires
- Hot plate
- Thermometers (2), ± 1°C
- Paper strips, 10cm x 1cm
- Magnetic stirrer
- Rubber gloves
- Apron
- Safety Goggles
Method
Method to prepare solutions
-
Concentration required (CuSO4): 0.99M
AMU of CuSO4: 159.61
So, 1.00M of CuSO4 has 159.61g of CuSO4
Hence 0.99M has: 159.61 x 0.99
= 158.01g ± 0.01g
Mix 158.01g ± 0.01g of CuSO4 in 100mL of distilled water. Use a magnetic stirrer if necessary
-
Use 100mL ± 1mL of 0.99M ± 0.01M of CuSO4 solution.
-
Concentration required (ZnSO4): 0.99M
AMU of ZnSO4: 161.44
So, 1.00M of CuSO4 has 161.44g of ZnSO4
Hence 0.99M has: 161.44 x 0.99
= 159.83g ± 0.01g
Mix 159.83g ± 0.01g of ZnSO4 in 100mL of distilled water. Use a magnetic stirrer if necessary
-
Use 100mL ± 1mL of 0.99M ± 0.01M of ZnSO4 solution.
-
Concentration required (KNO3): 1.99M
AMU of CuSO4: 101.11
So, 1.0M of CuSO4 has 101.11g of KNO3
Hence 1.99M has: 101.11 x 1.99
= 201.21g ± 0.01g
Mix 201.21g ± 0.01g of KNO3 in 100mL of distilled water. Use a magnetic stirrer if necessary
-
Use 30mL ± 1mL of 1.99M ± 0.01M of KNO3 solution.
-
Now put the paper strip (salt bridge) in the KNO3 solution and leave it for 30 seconds.
Method for investigation
- Before starting the experiments, all the materials should be acquired with all safety precautions
- Put the two beakers that have electrolytes on the hot plate.
- Now put the salt bridge between the beakers. Also, put the two thermometers in each container
- Connect the crocodile wires from the voltmeter to each electrode, but don’t put it in the half cells yet.
- Now turn on the hot plate and let the temperature increase from room temperature to 30°C
-
As soon as the temperature increases to 30°C, quickly insert the electrodes in the respective solutions (Cu in CuSO4 and Zn in ZnSO4) and record the voltage
- Remove the electrodes and clean and dry them.
- Now increase the temperature by a difference of 10°C i.e. 40°C, 50°C, 60°C, 70°C, 80°C and 90°C and repeat steps 5-7.
- After the experiment has been completed, put the cleaned materials back to their original place.
Raw Data Table
Processed Data
Data Processing
Note: For the sample calculation below, data point 2 has been used (30°C ± 1 °C).
Average Voltage = Trial 1 + Trial 2 + Trial 3
3
= 1.036 + 1.038 + 1.039
3
= 1.0376
= 1.038 V
Uncertainty of Average Voltage = Highest trial value – Lowest trial value
2
= 1.039 – 1.036
2
= 0.0015
= 0.002 V
= 1.038 V ± 0.002 V
Graph
Conclusion
Evaluation
Self Improvements
