An oxidation-reduction reaction in which 3 el | vedclass

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(A) The relationship between standard Gibbs free energy change and standard cell potential is given by the equation: $\Delta G^{\circ} = -nFE_{	ext{c

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$6$

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(A) The relationship between standard Gibbs free energy change and standard cell potential is given by the equation: $\Delta G^{\circ} = -nFE_{	ext{cell}}^{\circ}$.Given: $\Delta G^{\circ} = 17.37 \ kJ \ mol^{-1} = 17370 \ J \ mol^{-1}$,$n = 3$,and $F = 96500 \ C \ mol^{-1}$.Substituting the values: $17370 = -3 	imes 96500 	imes E_{	ext{cell}}^{\circ}$.$E_{	ext{cell}}^{\circ} = -\frac{17370}{3 	imes 96500} \ V$.$E_{	ext{cell}}^{\circ} = -\frac{17370}{289500} \ V \approx -0.06 \ V$.$E_{	ext{cell}}^{\circ} = -6 	imes 10^{-2} \ V$.Thus,the magnitude is $6 	imes 10^{-2} \ V$.

An oxidation-reduction reaction in which $3$ electrons are transferred has a $\Delta G^{\circ}$ of $17.37 \ kJ \ mol^{-1}$ at $25^{\circ} C$. The value of $E_{\text{cell}}^{\circ}$ (in $V$) is........ $\times 10^{-2} \ V$.
$(1 \ F = 96,500 \ C \ mol^{-1})$

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An oxidation-reduction reaction in which $3$ electrons are transferred has a $\Delta G^{\circ}$ of $17.37 \ kJ \ mol^{-1}$ at $25^{\circ} C$. The value of $E_{\text{cell}}^{\circ}$ (in $V$) is........ $\times 10^{-2} \ V$.$(1 \ F = 96,500 \ C \ mol^{-1})$