Three standard reduction half-equations and their standard electrode potentials are shown below:
V3+(aq)+e−⇌V2+(aq)Eθ=−0.26 V \text{V}^{3+}(\text{aq}) + \text{e}^- \rightleftharpoons \text{V}^{2+}(\text{aq}) \quad E^{\theta} = -0.26\text{ V} V3+(aq)+e−⇌V2+(aq)Eθ=−0.26 V Ti3+(aq)+e−⇌Ti2+(aq)Eθ=−0.37 V \text{Ti}^{3+}(\text{aq}) + \text{e}^- \rightleftharpoons \text{Ti}^{2+}(\text{aq}) \quad E^{\theta} = -0.37\text{ V} Ti3+(aq)+e−⇌Ti2+(aq)Eθ=−0.37 V Fe2+(aq)+2e−⇌Fe(s)Eθ=−0.44 V \text{Fe}^{2+}(\text{aq}) + 2\text{e}^- \rightleftharpoons \text{Fe}(\text{s}) \quad E^{\theta} = -0.44\text{ V} Fe2+(aq)+2e−⇌Fe(s)Eθ=−0.44 VWhich species is the strongest oxidizing agent under standard conditions?
Fe(s)\text{Fe}(\text{s})Fe(s)
V3+(aq)\text{V}^{3+}(\text{aq})V3+(aq)
Fe2+(aq)\text{Fe}^{2+}(\text{aq})Fe2+(aq)
V2+(aq)\text{V}^{2+}(\text{aq})V2+(aq)
