Given the half-reactions and $ \mathrm{E}_{\mathrm{red}}^{\circ} $ values below,determine which species is the best reducing agent.
$\begin{array}{ll}
\mathrm{MnO}_{4}-(a q)+8 \mathrm{H}^{+}(a q)+5 e^{-} \rightarrow \mathrm{Mn}^{2+}(a q)+4 \mathrm{H}_{2} \mathrm{O}(l) & \mathrm{E}_{\mathrm{red}=+1.512 \mathrm{~V}}^{\circ} \
4 \mathrm{H}^{+}(a q)+\mathrm{NO}_{3}-(a q)+3 e^{-} \rightarrow \mathrm{NO}(g)+2 \mathrm{H}_{2} \mathrm{O}(l) & \mathrm{E}_{\mathrm{red}=+0.964 \mathrm{~V}}^{\circ} \
\mathrm{Fe}^{3+}(a q)+e-\rightarrow \mathrm{Fe}^{2+}(s) & \mathrm{E}_{\mathrm{red}}^{\circ}=+0.771 \mathrm{~V} \
2 \mathrm{H}^{+}(a q)+2 e^{-} \rightarrow \mathrm{H}_{2}(g) & \mathrm{E}_{\text {red }}^{\circ}=0.000 \mathrm{~V}
\end{array}$

Question

Given the half-reactions and $ \mathrm{E}_{\mathrm{red}}^{\circ} $ values below,determine which species is the best reducing agent. 
$\begin{array}{ll}
\mathrm{MnO}_{4}-(a q)+8 \mathrm{H}^{+}(a q)+5 e^{-} \rightarrow \mathrm{Mn}^{2+}(a q)+4 \mathrm{H}_{2} \mathrm{O}(l) & \mathrm{E}_{\mathrm{red}=+1.512 \mathrm{~V}}^{\circ} \
4 \mathrm{H}^{+}(a q)+\mathrm{NO}_{3}-(a q)+3 e^{-} \rightarrow \mathrm{NO}(g)+2 \mathrm{H}_{2} \mathrm{O}(l) & \mathrm{E}_{\mathrm{red}=+0.964 \mathrm{~V}}^{\circ} \
\mathrm{Fe}^{3+}(a q)+e-\rightarrow \mathrm{Fe}^{2+}(s) & \mathrm{E}_{\mathrm{red}}^{\circ}=+0.771 \mathrm{~V} \
2 \mathrm{H}^{+}(a q)+2 e^{-} \rightarrow \mathrm{H}_{2}(g) & \mathrm{E}_{\text {red }}^{\circ}=0.000 \mathrm{~V}
\end{array}$

Quizplus · Accepted Answer

The Answer of Given the half-reactions and $ \mathrm{E}_{\mathrm{red}}^{\circ} $ values below,determine which species is the best reducing agent. 
$\begin{array}{ll}
\mathrm{MnO}_{4}-(a q)+8 \mathrm{H}^{+}(a q)+5 e^{-} \rightarrow \mathrm{Mn}^{2+}(a q)+4 \mathrm{H}_{2} \mathrm{O}(l) & \mathrm{E}_{\mathrm{red}=+1.512 \mathrm{~V}}^{\circ} \
4 \mathrm{H}^{+}(a q)+\mathrm{NO}_{3}-(a q)+3 e^{-} \rightarrow \mathrm{NO}(g)+2 \mathrm{H}_{2} \mathrm{O}(l) & \mathrm{E}_{\mathrm{red}=+0.964 \mathrm{~V}}^{\circ} \
\mathrm{Fe}^{3+}(a q)+e-\rightarrow \mathrm{Fe}^{2+}(s) & \mathrm{E}_{\mathrm{red}}^{\circ}=+0.771 \mathrm{~V} \
2 \mathrm{H}^{+}(a q)+2 e^{-} \rightarrow \mathrm{H}_{2}(g) & \mathrm{E}_{\text {red }}^{\circ}=0.000 \mathrm{~V}
\end{array}$

Given the Half-Reactions And Ered∘ \mathrm{E}_{\mathrm{red}}^{\circ} Ered∘​ Values Below,determine Which Species Is the Best Reducing Agent

Given the Half-Reactions And $\mathrm{E}_{\mathrm{red}}^{\circ}$ Values Below,determine Which Species Is the Best Reducing Agent