The cell potential for $\mathrm{Zn}\left|{\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right)\Vert {\mathrm{Sn}}^{\mathrm{x}+}\right|\mathrm{Sn}$ is $0.801\mathrm{V}$ at $298 \mathrm{K}$. The reaction quotient for the above reaction is ${10}^{-2}$. The number of electrons involved in the given electrochemical cell reaction is _____ .
(Given ${\mathrm{E}}_{{\mathrm{Zn}}^{2+}\mid \mathrm{Zn}}^0=-0.763 \mathrm{V},{\mathrm{E}}_{{\mathrm{Sn}}^{\mathrm{x}+}|\mathrm{Sn}}^0=+0.008 \mathrm{V}$ and $\frac{2.303\mathrm{RT}}{\mathrm{F}}=0.06 \mathrm{V}$)

The molar conductivity of a conductivity cell filled with $10$ moles of $20 \mathrm{mL} \mathrm{NaCl}$ solution is ${\mathrm{\Lambda }}_{\mathrm{m}1}$ and that of $20$ moles another identical cell heaving $80 \mathrm{mL} \mathrm{NaCl}$ solution is ${\mathrm{\Lambda }}_{\mathrm{m}2}$, The conductivities exhibited by these two cells are same.

The relationship between ${\mathrm{\Lambda }}_{\mathrm{m}2}$ and ${\mathrm{\Lambda }}_{\mathrm{m}1}$ is

The amount of charge in $\mathrm{F}$ (Faraday) required to obtain one mole of iron from ${\mathrm{Fe}}_3{\mathrm{O}}_4$ is

Round off the answer to the nearest integer.

Given below are two statements:

Statement I: For $\mathrm{KI}$, molar conductivity increases steeply with dilution.

Statement II: For carbonic acid, molar conductivity increases slowly with dilution. In the light of the above statements, choose the correct answer from the options given below

Match List-I with List-II.

Choose the correct answer from the options given below

For a cell, $\overline{)\mathrm{Cu}\left(\mathrm{s}\right)}{\mathrm{Cu}}^{2+}\left(\overline{)0.001\mathrm{M})}\left|{\mathrm{Ag}}^{+}\left(0.01\mathrm{M}\right)\right|\mathrm{Ag}\left(\mathrm{s}\right)\right.$the cell potential is found to be $0.43 \mathrm{V}$ at $298 \mathrm{K}$. The magnitude of standard electrode potential for ${\mathrm{Cu}}^{2+}|\mathrm{Cu}$ is____$\times {10}^{-2} \mathrm{V}$

$\left[\mathrm{Given}: {\mathrm{E}}_{{\mathrm{Ag}}^{+}/\mathrm{Ag}}^{\Theta }=0.80 \mathrm{V} \mathrm{and} \frac{2.303\mathrm{RT}}{\mathrm{F}}=0.06 \mathrm{V}\right]$

At $298 \mathrm{K}$, a $1$ litre solution containing $10 \mathrm{mmol}$ of ${\mathrm{Cr}}_2{\mathrm{O}}_7^{2-}$ and $100\mathrm{mmol}$ of ${\mathrm{Cr}}^{3+}$ shows a $\mathrm{pH}$ of $3.0$.

Given : ${\mathrm{Cr}}_2{\mathrm{O}}_7{}^{2-}\to {\mathrm{Cr}}^{3+};{\mathrm{E}}^0=1.330 \mathrm{V}$ and $\frac{2.303\mathrm{RT}}{\mathrm{F}}=0.059 \mathrm{V}$

The potential for the half cell reaction is $\mathrm{x}\times {10}^{-3} \mathrm{V}$ . The value of $\mathrm{x}$ is _____ .