Electrochemistry Questions

For the cell reaction:
2Fe
3+
(aq)+2I
−
(aq)→2Fe
2+
(aq)+I
2
​
(aq)
E
Cell
∘
​
=0.24V at 298K. The standard Gibbs energy (Δ
r
​
G
∘
) of the cell reaction is:

For a cell involving one electron E
cell
∘
​
=0.59V at 298K, the equilibrium constant for the cell reaction is:

The standard electrode potential ($E^{\circ }$) values of ${\text{Al}}^{3+}/\text{Al}$, ${\text{Ag}}^{+}/\text{Ag}$, ${\text{K}}^{+}/\text{K}$, and ${\text{Cr}}^{3+}/\text{Cr}$ are $-1.66\text{V}$, $0.80\text{V}$, $-2.93\text{V}$, and $-0.79\text{V}$ respectively. The correct decreasing order of the reducing power of the metal is:

Limiting molar conductivity of ${\text{NH}}_4\text{OH}$ (${\Lambda }_m^0({\text{NH}}_4\text{OH})$) is equal to:

Limiting molar conductivities for ${\text{H}}_2{\text{SO}}_4,{\text{K}}_2{\text{SO}}_4,$ and ${\text{CH}}_3\text{COOK}$ are $x,y,z$ respectively. From the data given above, it can be concluded that ${\Lambda }_m^0$ for ${\text{CH}}_3\text{COOH}$ will be: