Thanks An electrochemical cell, composed of an iron electrode (anode) immersed i

Question

Thanks An electrochemical cell, composed of an iron electrode (anode) immersed in 0.10 M Fe(NO3)2 and a silver electrode (cathode) immersed in 0.11 M AgNO3, was found to have a cell potential of 1.21 V. The standard reduction potential for the Ag'/Ag half-cell is + 0.80 V. The standard reduction potential for the Fe /Fe half-cell is -045 V. a. Write the half-cell reaction at the anode. b. Write the half-cell reaction at the cathode. c. Write the overall cell reaction. d. Determine the standard cell potential (e") using the standard reduction poten given above. · Determine the standard cell potential (e") using the Nernst equation.

Explanation / Answer

a) Half cell reaction for anode (iron will act as anode as it will undergo oxidation due to more negative reduction potential)

Fe(s) ---> Fe+2 + 2e

b) Half cell reaction for cathode

2×[Ag(aq) + e --> Ag(s)]

c) Overall reaction

Fe(s) + 2Ag+ --> Fe+2 + 2Ag(s)

d) The standard cell potential = E0cell

E0cell = E0cathode - E0anode

E0cell = 0.80 - (-0.45) = +1.25V

e) also

E0cell = Ecell - 0.0592 / n log Q

Q = [products]/[reactants]

Q = [Fe+2] / [Ag+]^2

Q = 0.10 / (0.11)^2 = 8.26

log Q = 0.917

E0cell = Ecell - 0.0296 log Q = 1.21 - 0.0296 X 0.917 = 1.18 volts

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