Which metal among the following has the strongest tendency to undergo oxidation?

Given the following standard electrode potentials:
$Cu^{+2} + 2e^{-} \to Cu$,$E^{o} = X_{1}$
$Cu^{+} + e^{-} \to Cu$,$E^{o} = X_{2}$
Calculate the standard electrode potential $E^{o}$ for the reaction: $Cu^{+2} + e^{-} \to Cu^{+}$

The standard reduction potentials of three metals $A, B,$ and $C$ are $+0.5 \, V, -3.0 \, V,$ and $-1.2 \, V$ respectively. What is the order of their reducing power?

$A$ standard hydrogen electrode has zero electrode potential because

Based on the data given below: $E^0_{Cr_2O_7^{2-}/Cr^{3+}} = 1.33 \text{ V}$,$E^0_{Cl_2/Cl^{-}} = 1.36 \text{ V}$,$E^0_{MnO_4^-/Mn^{2+}} = 1.51 \text{ V}$,$E^0_{Cr^{3+}/Cr} = -0.74 \text{ V}$. The strongest reducing agent is:

The standard electrode potential $({E^o})$ for $OCl^{-} / Cl^{-}$ and $Cl^{-} / \frac{1}{2}Cl_2$ respectively are $0.94 \ V$ and $-1.36 \ V$. The ${E^o}$ value for $OCl^{-} / \frac{1}{2}Cl_2$ will be ............... $V$.