Solution
= Solution
The more negative standard <reduction> potential identifies iron as the species more readily oxidized. Combining $\mathrm{Fe\to Fe^{2+}+2e^-}$ with $\mathrm{Sn^{2+}+2e^-\to Sn}$ gives the spontaneous standard <galvanic cell> reaction
$$
\boxed{\mathrm{Fe(s)+Sn^{2+}(aq)\longrightarrow Fe^{2+}(aq)+Sn(s)}}.
$$
The <electron> balance is two per reaction, and the activities of the pure metals are unity.