Question Bank [2022] — Chemistry STD 12 Science — Question
Maharashtra BoardEnglish MediumSTD 12 ScienceChemistryQuestion Bank [2022]2 Marks
Question
Derive the relationship between standard cell potential and equilibrium constant of cell reaction.
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Answer
The relation between standard Gibbs energy change of cell reaction and standard cell potential is given by $ -\Delta G ^{\circ}=- nF E _{\text {cell }}^{\circ} \cdots(1) $
The relation between standard Gibbs energy change of a chemical reaction and its equilibrium constant as given in thermodynamics is: $ \Delta G^{\circ}=-R T \ln K \cdots(2) $
Combining equations (1) and (2), we have $ -n F E_{\text {cell }}^{\circ}=- RT \ln K $ $ \therefore E _{\text {cell }}^{\circ}=\frac{ RT }{ nF } \ln K $ $ =\frac{2.303 RT }{ nF } \log _{10} K $ $ =\frac{0.0592}{ n } \log _{10} K \text { at } 25^{\circ} C $
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