If the free-energy change for the reaction is -87.5 kJ and the cell potential is equal to 0.18 V, how many moles of electrons are used in the reaction? Given: F = $96,468 \mathrm {~J} / (\mathrm { V } \cdot \mathrm { mol } )$ .

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The Answer of If the free-energy change for the reaction is -87.5 kJ and the cell potential is equal to 0.18 V, how many moles of electrons are used in the reaction? Given: F = $96,468 \mathrm {~J} / (\mathrm { V } \cdot \mathrm { mol } )$ .

If the Free-Energy Change for the Reaction Is -87 96,468 J/(V⋅mol)96,468 \mathrm {~J} / (\mathrm { V } \cdot \mathrm { mol } )96,468 J/(V⋅mol)

If the Free-Energy Change for the Reaction Is -87 $96,468 \mathrm {~J} / (\mathrm { V } \cdot \mathrm { mol } )$