The table below lists the standard electrode potentials (EθE^\thetaEθ) for several half-cells:
Half-cell ReactionEθ/VCe4+(aq)+e−⇌Ce3+(aq)+1.70Cl2(g)+2e−⇌2Cl−(aq)+1.36Fe3+(aq)+e−⇌Fe2+(aq)+0.77Cu2+(aq)+2e−⇌Cu(s)+0.34Sn2+(aq)+2e−⇌Sn(s)−0.14 \begin{array}{c|c} \text{Half-cell Reaction} & E^\theta / \text{V} \\ \hline \text{Ce}^{4+}(\text{aq}) + \text{e}^- \rightleftharpoons \text{Ce}^{3+}(\text{aq}) & +1.70 \\ \text{Cl}_2(\text{g}) + 2\text{e}^- \rightleftharpoons 2\text{Cl}^-(\text{aq}) & +1.36 \\ \text{Fe}^{3+}(\text{aq}) + \text{e}^- \rightleftharpoons \text{Fe}^{2+}(\text{aq}) & +0.77 \\ \text{Cu}^{2+}(\text{aq}) + 2\text{e}^- \rightleftharpoons \text{Cu}(\text{s}) & +0.34 \\ \text{Sn}^{2+}(\text{aq}) + 2\text{e}^- \rightleftharpoons \text{Sn}(\text{s}) & -0.14 \end{array} Half-cell ReactionCe4+(aq)+e−⇌Ce3+(aq)Cl2(g)+2e−⇌2Cl−(aq)Fe3+(aq)+e−⇌Fe2+(aq)Cu2+(aq)+2e−⇌Cu(s)Sn2+(aq)+2e−⇌Sn(s)Eθ/V+1.70+1.36+0.77+0.34−0.14Based on these data, which of the following chemical reactions is thermodynamically feasible under standard conditions?
2Fe3+(aq)+2Cl−(aq)→2Fe2+(aq)+Cl2(g)2\text{Fe}^{3+}(\text{aq}) + 2\text{Cl}^-(\text{aq}) \rightarrow 2\text{Fe}^{2+}(\text{aq}) + \text{Cl}_2(\text{g})2Fe3+(aq)+2Cl−(aq)→2Fe2+(aq)+Cl2(g)
Cu2+(aq)+2Ce3+(aq)→Cu(s)+2Ce4+(aq)\text{Cu}^{2+}(\text{aq}) + 2\text{Ce}^{3+}(\text{aq}) \rightarrow \text{Cu}(\text{s}) + 2\text{Ce}^{4+}(\text{aq})Cu2+(aq)+2Ce3+(aq)→Cu(s)+2Ce4+(aq)
2Fe3+(aq)+Sn(s)→2Fe2+(aq)+Sn2+(aq)2\text{Fe}^{3+}(\text{aq}) + \text{Sn}(\text{s}) \rightarrow 2\text{Fe}^{2+}(\text{aq}) + \text{Sn}^{2+}(\text{aq})2Fe3+(aq)+Sn(s)→2Fe2+(aq)+Sn2+(aq)
Sn2+(aq)+Cu(s)→Sn(s)+Cu2+(aq)\text{Sn}^{2+}(\text{aq}) + \text{Cu}(\text{s}) \rightarrow \text{Sn}(\text{s}) + \text{Cu}^{2+}(\text{aq})Sn2+(aq)+Cu(s)→Sn(s)+Cu2+(aq)