Based on the half-reactions and their respective standard reduction potentials below,what is the standard cell potential for the reaction that is expected to occur? Fe³⁺(aq) + e^- → Fe²⁺(aq) 0.77 V
Sn⁴⁺(aq) + 2 e^- → Sn²⁺(aq) 0.15 V
Pb²⁺(aq) + 2 e^- → Pb(s) -0.13 V

Question

Quizplus · Accepted Answer

The standard cell potential ($E^\circ_{cell}$) is calculated by subtracting the standard reduction potential of the anode ($E^\circ_{anode}$) from the standard reduction potential of the cathode ($E^\circ_{cathode}$). Here, Fe$^{3+}$ to Fe$^{2+}$ (0.77 V) acts as the cathode reaction, and Sn$^{4+}$ to Sn$^{2+}$ (0.15 V) acts as the anode reaction. Thus, $E^\circ_{cell} = 0.77 V - 0.15 V = 0.62 V$. However, given the options, it seems there might be a misunderstanding in the interpretation of the question or a typographical error in the options or explanation. The correct calculation based on the provided potentials and assuming the standard reaction setup would typically involve subtracting the lower potential from the higher potential.

Based on the Half-Reactions and Their Respective Standard Reduction Potentials