Nernst Equation

Consider the cell at 25°C
Zn | Zn²?(aq), (1M) Fe³?(aq), Fe²?(aq) | Pt(s)
The fraction of total iron present as Fe³? ion at the cell potential of 1.500V is x * 10?². The value of x is ______ (Nearest integer).
(Given: E?(Fe³?/Fe²?) = 0.77V, E?(Zn²?/Zn) = -0.76V)

Emf of the following cell at 298 K in V is x * 10^-2.

$Zn\left|Z{n}^{2+}\left(0.1M\right)\right|\left|A{g}^{+}\left(0.01M\right)\right|Ag$

The value of x is………… (Rounded off to the nearest integer)

$\left[Given:E_{Z{n}^{2+}/Zn}^0=-0.76V;E_{A{g}^{+}/Ag}^0=+0.80V;\frac{2.303RT}{F}=0.059\right]$

The magnitude of the change in oxidizing power of the $Mn{O}_4^{-}/M{n}^{2+}$  couple is x * 10^-4 V, if the H⁺ concentration is decrease from 1M to 10^-4M at 25°C (Assume concentration of   $Mn{O}_4^{-}$ and Mn²⁺ to be same on change in H⁺ concentration). The value of x is………………… (Rounded off to the nearest integer)

[Given : $\frac{2.303RT}{F}=0.059$ ]

For a cell, $Cu\left(s\right)\left|C{u}^{2+}\left(0.001M\right)\right|\left|A{g}^{+}\left(0.01M\right)\right|Ag\left(s\right)$  

The cell potential is found to be 0.43V at 298 K. The magnitude of standard electrode potential for Cu²⁺ / Cu is______________ × 10^-2V.

$\left[Given:E_{A{g}^{+}/Ag}^{\Theta }=0.80Vand\frac{2.303RT}{F}=0.06V\right]$