An electrolytic cell is set up using inert platinum electrodes immersed in a \(1.0\text{ M }\text{NaBr(aq)}\) solution at \(298\text{ K}\). A direct current is applied to drive the nonspontaneous process.

Half-reaction	\(E^\circ\text{ at } 298\text{ K}\)
\(\text{Na}^+\text{(aq)} + e^- \rightarrow \text{Na(s)}\)	\(-2.71\text{ V}\)
\(2\text{H}_2\text{O}(l) + 2e^- \rightarrow \text{H}_2\text{(g)} + 2\text{OH}^-\text{(aq)}\)	\(-0.83\text{ V}\)
\(\text{Br}_2(l) + 2e^- \rightarrow 2\text{Br}^-\text{(aq)}\)	\(+1.07\text{ V}\)
\(\text{O}_2\text{(g)} + 4\text{H}^+\text{(aq)} + 4e^- \rightarrow 2\text{H}_2\text{O}(l)\)	\(+1.23\text{ V}\)

Based on the standard reduction potentials in the table, which of the following correctly identifies the chemical species reduced at the cathode and the chemical species oxidized at the anode?