CuSO4-1.0m ZnSO4-1.0M Kcl-1.0M One beakers with 45mL of zinc second beakerwith c

Question

CuSO4-1.0m

ZnSO4-1.0M

Kcl-1.0M

One beakers with 45mL of zinc second beakerwith copper sulfate
Put the salt bridge(1.5 inches folded of filter paper soak in potassium chloride) into place by submerging 1 end in copper sulfate and the other end in zinc sulfate. Clip a piece of zinch to one end of the jumper cable and clip a piece of copper onto the other. Place the copper into copper sulfate solution ans the zinc into the zinc sulfate solution.

Exercise 1: Construction of a Galvanic Cell

Data Table 1. Spontaneous Reaction Observations.

Metal in Solution

Observations

Zinc in Copper Sulfate

Zinc turns black

Copper in Zinc Sulfate

No change occured

Data Table 2. Voltmeter Readings.

Time (minutes)

Voltmeter Reading (Volts)

0

1.07

15

1.08

30

1.08

45

1.08

60

1.08

75

1.08

90

1.08

105

1.08

120

1.05

135

1.04

Data Table 3. Standard Cell Potential.

Equation

E°(Volts)

Oxidation Half-Reaction

Zn(s) ------> Zn2+(aq) + 2e-

0.76V

Reduction Half-Reaction

Cu2+(aq) + 2e- -------> Cu(s)

0.13V

Redox Reaction

Zn(s) + CuSO4(aq) -----------> ZnSO4(aq) + Cu(s)

0.89V

Questions

What were the concentrations of the solutions (zinc solution, copper solution, and salt bridge)? Were the concentrations consistent with those of standard state conditions? Explain your answer.

Was the amount of electric energy produced in your galvanic cell consistent with the standard cell potential of the reaction (as calculated in Data Table 3)? Hypothesize why it was or was not consistent.

Was there evidence of electron transfer from the anode to the cathode? Use your data in Data Table 2 to explain your answer.

For the following redox reaction in a galvanic cell, write the oxidation half-reaction and the reduction-half reaction, and calculate the standard cell potential of the reaction. Use Table 1 in the Background as needed. Explain how you identified which half-reaction is the oxidizer and which is the reducer. Show all of your work.

Metal in Solution

Observations

Zinc in Copper Sulfate

Zinc turns black

Copper in Zinc Sulfate

No change occured

Explanation / Answer

Questions:

a) The concentrations of solutions would not be changed if we are taking Zn/ZnSO4 // CusO4/Cu cell. Because how many ions are coming from Zn to ZnSO4. That many ions again reproduced due to an equilibrium reaction.

So all concentrations are - CuSO4 = 1 M, ZnSO4 = 1M

b) Yes , the concentrations are consistent through out the experiment. It was proved by the potential values occured in the experiment.

c) The obtained values are consistent and galvanic meter values are consistent and supporting to calculate the values of total cell potentials. If we add, both oxidation and reduction potential values from Data table:3 we get the cell potential. 0.89 V (0.76+0.13). So amount of energy produced in cell is consistent through out the experiment and its proportional to total cell potential.

d) Yes, because if there is no electron transfer from anode to cathode in the cell there is no generation electrical energy. The values in Galvano meter(Data table:2) showing that the electrons are tranfering from anode to cahode.

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