Chemistry

Problem

The following standard half-reactions are available at 298 K. 1. Cu

^{2+}

+ 2 e

^{-}

→ Cu(s)

E^{\circ}=+0.34\,\text{V}

2. Sn

^{4+}

+ 2 e

^{-}

→ Sn

^{2+}

E^{\circ}=+0.15\,\text{V}

Which statement correctly identifies the cathode process for the spontaneous cell formed from these two half-reactions? a)

\text{Sn}^{4+}\text{ is reduced to Sn}^{2+}\text{ at the cathode.}

\text{Cu(s) is oxidized to Cu}^{2+}\text{ at the cathode.}

\text{Cu}^{2+}\text{ is reduced to Cu(s) at the cathode.}

\text{Sn}^{2+}\text{ is oxidized to Sn}^{4+}\text{ at the cathode.}