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Question

Which of the following relation(s) is/are correct?
Here,
ΔG=Change in Gibbs' free energyn=no. of moles of electron transferred in a reactionF=Faraday constantEcell=Cell potential or emf

A
ΔG=Maximum useful work
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B
ΔG=Minimum useful work
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C
All of the above
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D
nΔG=FEcell
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Solution

The correct option is A ΔG=Maximum useful work
For a spontaneous reaction
ΔG<0
The free energy change ΔG (a thermochemical quantity) and the cell potential Ecell (an electrochemical quantity),both measure the driving force of a chemical reaction
Larger the decrease in free energy, greater would be the emf.

Mathematically,
ΔG=Maximum useful work
ΔG=Welectrical
ΔG=Qtotal×Ecell
Here ,
Qtotal=Total charge
Qtotal=nF

n=no. of moles of electron transferred in a reactionF=Faraday constant

Faraday constant is the charge on 1 mol of electrons

So,
ΔG=nF×Ecell
Charge on one electron=1.6×1019 C
Charge on one mol of electrons (F)=1.6×1019×NA CF=1.6×1019×6.022×1023=96487 C

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