Standard reduction potentials of the half reactions are given below :
F_2(g) + 2e^$$-$$ $$ \to $$ 2F^$$-$$_(aq) ;   E^o = + 2.85 V
Cl_2(g) + 2e^$$-$$ $$ \to $$ 2Cl^$$-$$_(aq) ;   E^o = + 1.36 V
Br_2(l) + 2e^$$-$$ $$ \to $$ 2Br^$$-$$_(aq) ;   E^o = + 1.06 V
I_2(s) + 2e^$$-$$ $$ \to $$ 2I^$$-$$_(aq) ;  E^o = + 0.53 V

The strongest oxidising and reducing agents 23 respectively are

Limiting molar conductivity of NH₄OH
$$\left[ {} \right.$$i.e.  $$\Lambda _{m\left( {N{H_4}OH} \right)}^0$$$$\left. {} \right]$$ is equal to

A solution contains Fe²⁺, Fe³⁺ and I^$$-$$ ions. This solution was treated with iodine at 35^oC. E^o for Fe³⁺/Fe²⁺ is + 0.77 V and E^o for I₂/2I^$$-$$ = 0.536 V.
The favourable redox reaction is

Standard electrode potential of three metals X, Y and Z are $$-$$1.2 V, + 0.5 V and $$-$$ 3.0 V respectively. The reducing power of these metals will be