Redox reactions play a pivotal role in chemistry and biology. The values of standard redox potential

Question

Redox reactions play a pivotal role in chemistry and biology. The values of standard redox potential ( $E^{\circ}$ ) of two halfcell reactions decide which way the reaction is expected to proceed. A simple example is a Daniell cell in which zinc goes into solution and copper gets deposited. Given below are a set of half-cell reactions (acidic medium) along with their $E^{\circ}(\mathrm{V}$ with respect to normal hydrogen electrode) values. 
$
\begin{array}{ll}
\mathrm{I}_2+2 e^{-} ightarrow 2 \mathrm{I}^{-} & E^{\circ}=0.54 \
\mathrm{Cl}_2+2 e^{-} ightarrow 2 \mathrm{Cl}^{-} & E^{\circ}=1.36 \
\mathrm{Mn}^{3+}+e^{-} ightarrow \mathrm{Mn}^{2+} & E^{\circ}=1.50 \
\mathrm{Fe}^{3+}+e^{-} ightarrow \mathrm{Fe}^{2+} & E^{\circ}=0.77 \
\mathrm{O}_2+4 \mathrm{H}^{+}+4 e^{-} ightarrow 2 \mathrm{H}_2 \mathrm{O} & E^{\circ}=1.23
\end{array}
$

Professor PC Thomas Classes · Answer

See detailed solution for explanation.