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(D) An oxidizing agent is a species that gets reduced,meaning it has a higher reduction potential.The given reactions are oxidation half-reactions. We

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$Fe^{3+}$

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(D) An oxidizing agent is a species that gets reduced,meaning it has a higher reduction potential.The given reactions are oxidation half-reactions. We must convert them to reduction potentials:$1. [Fe(CN)_6]^{3-} + e^- 	o [Fe(CN)_6]^{4-}, E^o_{red} = +0.35 \ V$$2. Fe^{3+} + e^- 	o Fe^{2+}, E^o_{red} = +0.77 \ V$Comparing the reduction potentials,$E^o_{red}(Fe^{3+}/Fe^{2+}) = +0.77 \ V$ is greater than $E^o_{red}([Fe(CN)_6]^{3-}/[Fe(CN)_6]^{4-}) = +0.35 \ V$.Therefore,$Fe^{3+}$ is a stronger oxidizing agent than $[Fe(CN)_6]^{3-}$.

From the given values,which one is a strong oxidizing agent?
$[Fe(CN)_6]^{4-} \to [Fe(CN)_6]^{3-} + e^-, E^o = -0.35 \ V$
$Fe^{2+} \to Fe^{3+} + e^-, E^o = -0.77 \ V$

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On the basis of the following $E^o$ values,the strongest oxidizing agent is:
$[Fe(CN)_6]^{4-} \to [Fe(CN)_6]^{3-} + e^-; E^o = -0.35 \ V$
$Fe^{2+} \to Fe^{3+} + e^-; E^o = -0.77 \ V$

For the cell reaction,$2 Al_{(s)} + 3 Cu^{2+}_{(aq)} \rightarrow 2 Al^{3+}_{(aq)} + 3 Cu_{(s)}$. If $\Delta G^{\circ} = -1158 \ kJ$,what is $E^{\circ}_{cell}$ (in $V$)?

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From the given values,which one is a strong oxidizing agent?$[Fe(CN)_6]^{4-} \to [Fe(CN)_6]^{3-} + e^-, E^o = -0.35 \ V$$Fe^{2+} \to Fe^{3+} + e^-, E^o = -0.77 \ V$