The standard reduction potentials for the and electrodes are and respectively. For the specific cell — Electrochemistry Chemistry Question

💡 Solution & Explanation

In the provided redox reaction, $Sn$ undergoes oxidation to $Sn^{2+}$ (acting as the anode) and $Fe^{2+}$ undergoes reduction to $Fe$ (acting as the cathode). The standard cell potential is computed as $E^\circ_{cell} = E^\circ_{cathode} - E^\circ_{anode} = E^\circ_{Fe^{2+}/Fe} - E^\circ_{Sn^{2+}/Sn} = -0.44\text{ V} - (-0.14\text{ V}) = -0.30\text{ V}$. The negative sign confirms the reaction is non-spontaneous as written.