Red ox reaction play a pivotal role in chemistry and biology.The values of standard redox potential (E⁰ ) of two half-cell reactions decide which way the reaction is expected to proceed, A simple example is a Daniel 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 with E⁰ respect to normal hydrogen electrode values. Using this data obtain the correct explanations to following Questions.
$\begin{array}{l} I_{2} + 2 e^{-} \to 2 I^{-} E^{0} = 0 .54 \\ {Cl}_{2} + 2 e^{-} \to 2 {Cl}^{-} E^{0} = 1 .36 \\ {Mn}^{3 +} + e^{-} \to Mn E^{0} = 1 .50 \\ {Fe}^{3 +} + e^{-} \to {Fe}^{2 +} E^{0} = 0 .77 \\ O_{2} + 4 H^{+} + 4 e^{-} \to 2 H_{2} O E^{0} = 1 .23 \end{array}$

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