Using the standard electrode potential data provided below, predict which of the following redox reactions will occur spontaneously under standard conditions.
Fe3+(aq)+e−⇌Fe2+(aq)E⊖=+0.77 VI2(aq)+2e−⇌2I−(aq)E⊖=+0.54 VAg+(aq)+e−⇌Ag(s)E⊖=+0.80 VBr2(aq)+2e−⇌2Br−(aq)E⊖=+1.09 V \begin{array}{rcll} \text{Fe}^{3+}(aq) + e^- & \rightleftharpoons & \text{Fe}^{2+}(aq) & E^\ominus = +0.77\text{ V} \\ \text{I}_2(aq) + 2e^- & \rightleftharpoons & 2\text{I}^-(aq) & E^\ominus = +0.54\text{ V} \\ \text{Ag}^+(aq) + e^- & \rightleftharpoons & \text{Ag}(s) & E^\ominus = +0.80\text{ V} \\ \text{Br}_2(aq) + 2e^- & \rightleftharpoons & 2\text{Br}^-(aq) & E^\ominus = +1.09\text{ V} \end{array} Fe3+(aq)+e−I2(aq)+2e−Ag+(aq)+e−Br2(aq)+2e−⇌⇌⇌⇌Fe2+(aq)2I−(aq)Ag(s)2Br−(aq)E⊖=+0.77 VE⊖=+0.54 VE⊖=+0.80 VE⊖=+1.09 VThe oxidation of Fe2+(aq)\text{Fe}^{2+}(aq)Fe2+(aq) by I2(aq)\text{I}_2(aq)I2(aq) to form Fe3+(aq)\text{Fe}^{3+}(aq)Fe3+(aq) and I−(aq)\text{I}^-(aq)I−(aq)
The oxidation of Br−(aq)\text{Br}^-(aq)Br−(aq) by Ag+(aq)\text{Ag}^+(aq)Ag+(aq) to form Br2(aq)\text{Br}_2(aq)Br2(aq) and Ag(s)\text{Ag}(s)Ag(s)
The oxidation of I−(aq)\text{I}^-(aq)I−(aq) by Fe3+(aq)\text{Fe}^{3+}(aq)Fe3+(aq) to form I2(aq)\text{I}_2(aq)I2(aq) and Fe2+(aq)\text{Fe}^{2+}(aq)Fe2+(aq)
The oxidation of Ag(s)\text{Ag}(s)Ag(s) by Fe3+(aq)\text{Fe}^{3+}(aq)Fe3+(aq) to form Ag+(aq)\text{Ag}^+(aq)Ag+(aq) and Fe2+(aq)\text{Fe}^{2+}(aq)Fe2+(aq)