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Consider the voltaic cell composed of a Mn/Mn2+ electrode and a Fe/Fe2+ electrode. Calculate the concentration...

Consider the voltaic cell composed of a Mn/Mn2+ electrode and a Fe/Fe2+ electrode. Calculate the concentration of Fe2+ if the concentration of Mn2+ is 0.010 M and Ecell is 0.78V.

Expert Solution

Standard Electrode reduction potential of Mn/Mn2+ = -1.18 V ( Anode, with higher -ve potential)

Standard Electrode reduction potential of Fe/Fe2+ = -0.44 V ( cathode, with lower -ve potential)

Standard Cepotential ,

= -0.44 - ( -1.18)

= + 0.74 V

Given cell potential at given concentratios , 0.78 V

The cell redox reaction is written as ---

BY Nernst equation the cel potential and metnioned concetrations of electrodes are related as -------

n= 2 electrons involved in the above reaction

R = 8.314 j/mol.K

F = 96485 C/mol

The concetration of Mn and Fe in their states are unity.

T = 298 K ( laboratory room temperature 25^0 C)

-------------------------------------------------------------------------------------------------------------------------------------------------

Dimensional analysis is fulfilled. ( volt = j/C) . All units balanced.

log 0.01 M - log[Fe^2+] = -0.001182

log[Fe^2+] = log 0.01 M + 0.001182

= -2 + 0.001182

= -1.9988

[Fe^2+] = 10^-1.9988

= 0.01002 M

queen_honey_blossom answered 2 years ago

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