The `E_(cell)` for a given cell is `1.2346` and `1.2340V` at `300K ` and `310K`, respectively. Calculate the change in entropy during the cell reaction if the redox change involves three electrons.A. `-17.37 J K^(-1)`B. `+17.37 J K ^(-1)`C. `173.7J K^(-1)`D. `5.79 J K^(-1)`

The `E_(cell)` for a given cell is `1.2346` and `1.2340V` at `300K ` a

1.	The `E_(cell)` for a given cell is `1.2346` and `1.2340V` at `300K ` and `310K`, respectively. Calculate the change in entropy during the cell reaction if the redox change involves three electrons.A. `-17.37 J K^(-1)`B. `+17.37 J K ^(-1)`C. `173.7J K^(-1)`D. `5.79 J K^(-1)`
Answer» Correct Answer - a By `DeltaS=(DeltaH-DeltaG)/(T),` `DeltaH=-nF[E-T((delE)/(delT))_(P)]` and `DeltaG=-nEF` `DeltaS=-nF((delE)/(delT))_(p)=3xx96500xx(-(0.0006)/(10))` `=-17.37 J K^(-1)`

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The `E_(cell)` for a given cell is `1.2346` and `1.2340V` at `300K ` and `310K`, respectively. Calculate the change in entropy during the cell reaction if the redox change involves three electrons.A. `-17.37 J K^(-1)`B. `+17.37 J K ^(-1)`C. `173.7J K^(-1)`D. `5.79 J K^(-1)`

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