Use the standard electrode potential data in the table to determine which species is the strongest oxidizing agent among the choices provided.
Half-equationEθ/VCe4+(aq)+e−⇌Ce3+(aq)+1.70MnO4−(aq)+8H+(aq)+5e−⇌Mn2+(aq)+4H2O(l)+1.51Cl2(g)+2e−⇌Cl−(aq)+1.36Fe3+(aq)+e−⇌Fe2+(aq)+0.77 \begin{array}{lc} \text{Half-equation} & E^\theta / \text{V} \\ \hline \text{Ce}^{4+}(\text{aq}) + \text{e}^- \rightleftharpoons \text{Ce}^{3+}(\text{aq}) & +1.70 \\ \text{MnO}_4^-(\text{aq}) + 8\text{H}^+(\text{aq}) + 5\text{e}^- \rightleftharpoons \text{Mn}^{2+}(\text{aq}) + 4\text{H}_2\text{O}(\text{l}) & +1.51 \\ \text{Cl}_2(\text{g}) + 2\text{e}^- \rightleftharpoons \text{Cl}^-(\text{aq}) & +1.36 \\ \text{Fe}^{3+}(\text{aq}) + \text{e}^- \rightleftharpoons \text{Fe}^{2+}(\text{aq}) & +0.77 \end{array} Half-equationCe4+(aq)+e−⇌Ce3+(aq)MnO4−(aq)+8H+(aq)+5e−⇌Mn2+(aq)+4H2O(l)Cl2(g)+2e−⇌Cl−(aq)Fe3+(aq)+e−⇌Fe2+(aq)Eθ/V+1.70+1.51+1.36+0.77Ce3+(aq)\text{Ce}^{3+}(\text{aq})Ce3+(aq)
MnO4−(aq)\text{MnO}_4^-(\text{aq})MnO4−(aq)
Mn2+(aq)\text{Mn}^{2+}(\text{aq})Mn2+(aq)
Fe3+(aq)\text{Fe}^{3+}(\text{aq})Fe3+(aq)
