$\mathrm{Emf}$ of the following cell at $298 \mathrm{K}$ in $\mathrm{V}$ is $\mathrm{x}\times {10}^{-2}$

$\mathrm{Zn}\left|{\mathrm{Zn}}^{2+}\left(0.1\mathrm{M}\right)\Vert {\mathrm{Ag}}^{+}\left(0.01\mathrm{M}\right)\right|\mathrm{Ag}$

The value of $\mathrm{x}$ is ________________ (Rounded off to the nearest integer)

$\left[\mathrm{Given}: {\mathrm{E}}_{{\mathrm{Zn}}^{2+}/\mathrm{Zn}}^{\theta }=-0.76 \mathrm{V}; {\mathrm{E}}_{{\mathrm{Ag}}^{+}/\mathrm{Ag}}^{\theta }=+0.80 \mathrm{V}; \frac{2.303\mathrm{RT}}{\mathrm{F}}=0.059\right]$

Consider the following reaction

${\mathrm{MnO}}_4^{-}+8{\mathrm{H}}^{+}+5{\mathrm{e}}^{-}\to {\mathrm{Mn}}^{+2}+4{\mathrm{H}}_2\mathrm{O} ,\mathrm{E}°=1.51 \mathrm{V}$

The quantity of electricity required in Faraday to reduce five moles of ${\mathrm{MnO}}_4^{-}$ is              

For the galvanic cell,

$\mathrm{Zn}\left(\mathrm{s}\right)+{\mathrm{Cu}}^{2+}(0.02\mathrm{M})\to {\mathrm{Zn}}^{2+}(0.04\mathrm{M})+\mathrm{Cu}\left(\mathrm{s}\right)$

${\mathrm{E}}_{\mathrm{cell} }=\dots \times {10}^{-2} \mathrm{V}$ (Nearest integer)

$\left[\mathrm{Use}:{\mathrm{E}}^0\mathrm{Cu}/{\mathrm{Cu}}^{2+}=-0.34 \mathrm{V},{\mathrm{E}}_{\mathrm{Zn}/{\mathrm{Zn}}^2+}=+0.76 \mathrm{V},\frac{2.303\mathrm{RT}}{\mathrm{F}}=0.059 \mathrm{V}\right]$

Given below are two statements:
Statement I : The limiting molar conductivity of $\mathrm{KCl}$ (strong electrolyte) is higher compared to that of $\mathrm{CH}_{3} \mathrm{COOH}$ (weak electrolyte).
Statement II : Molar conductivity decreases with decrease in concentration of electrolyte.

In the light of the above statements, choose the most appropriate answer from the options given below:

Consider the cell at $25°\mathrm{C}$

$\mathrm{Zn}\left|{\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right),\left(1 \mathrm{M}\right)\Vert {\mathrm{Fe}}^{3+}\left(\mathrm{aq}\right),{\mathrm{Fe}}^{2+}\left(\mathrm{aq}\right)\right|\mathrm{Pt}\left(\mathrm{s}\right)$

The fraction of total iron present as ${\mathrm{Fe}}^{3+}$ ion at the cell potential of $1.500 \mathrm{V}$ is $\mathrm{x}\times {10}^{-2}$. The value of $\mathrm{x}$ is ______. (Nearest integer)

$\mathrm{Given}:\hspace{0.17em}{{\mathrm{E}}^{\circ }}_{{\mathrm{Fe}}^{3+}|{\mathrm{Fe}}^{2+}}=0.77\mathrm{V}, \hspace{0.17em}{{\mathrm{E}}^{\circ }}_{{\mathrm{Zn}}^{2+}|\mathrm{Zn}}=-0.76\mathrm{V}$

The magnitude of the change in oxidising power of the ${\mathrm{MnO}}_4^{-}/{\mathrm{Mn}}^{2+}$ couple is $\mathrm{x}\times {10}^{-4} \mathrm{V}$ if the ${\mathrm{H}}^{+}$ concentration is decreased from $1 \mathrm{M}$ to ${10}^{-4}\mathrm{M}$ at $25°\mathrm{C}.$ (Assume concentration of ${\mathrm{MnO}}_4^{-}$ and ${\mathrm{Mn}}^{2+}$ to be same on change in ${\mathrm{H}}^{+}$ concentration). The value of $\mathrm{x}$ is __________.

(Rounded off to the nearest integer)

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

Assume a cell with the following reaction ${\mathrm{Cu}}_{\left(\mathrm{s}\right)}+2{\mathrm{Ag}}^{+}\left(1\times {10}^{-3}\mathrm{M}\right)\to {\mathrm{Cu}}^{2+}(0.250\mathrm{M})+2{\mathrm{Ag}}_{\left(\mathrm{s}\right)}$
${\mathrm{E}}_{\mathrm{cell} }^{\circ }=2.97 \mathrm{V}$

${\mathrm{E}}_{\mathrm{cell} }$ for the above reaction is $\underline{ }$  $\mathrm{V}.$

(Nearest integer)

$[$ Given : $\log 2.5=0.3979, \mathrm{T}=298 \mathrm{K}]$