please help me this Electrochemical cell lab lead bar+lead(2)nitrate(0.10M), Zin

Question

please help me this Electrochemical cell lab

lead bar+lead(2)nitrate(0.10M), Zinc sulfite(0.10M)+zinc bar.

Lead and Zinc Voltaic Cell Write the cell diagram (notation) for the cell reaction and complete die table below. Write the equation far the reaction that occurs in the cell, write it as an equilibrium. Write the equilibrium constant expression for the cell reaction. Calculate the potential far the cell used in this part of the experiment. Shaw your calculations here and report in Volts (V). Transfer your answer to the table above in milliVolts (mV). Use the standard cell potential to calculate the free energy change for the cell reaction under standard conditions. Use the standard cell paternal to calculate the equilibrium constant for the cell reaction under standard conditions. Complete the cell sketch below.

Explanation / Answer

ANSWER:

1. Cell Notation is given below

Pb,PbNO3 (0.1M)II ZnSO3 (0.1M), Zn

Error can be calculatd only when measured value of valtage is given. But you have not give the value that you got from your experiment.

2. Equation

Zn(s) + Pb2+(aq)<---------> Zn2+(aq) + Pb(s)

3. Equilibrium constant K = [Pb2+][Zn]/[Pb][Zn2+] = [Pb2+]/[Zn2+]

Because [Zn] and [Pb] is taken as unity.

4. Potential of the cell E = Eocathod - Eoanode

E = -0.126 - (-0.763) = - 0.126 + 0.763 = 0.637V

5.) Go = - nFEo

n = no. of electrons involved in the reation

F = faraday constant = 96485C/mol

Go = - 2X96485 X 0.637

Go = - 122.9KJ Negative sign indicates energy is released.

6) - Go = nFEo = RTlnK

122900 = 8.314 X 298 X lnK

lnK = 49.6

K = 3.47 X 1021

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