Nernst Equation and its Applications

$\left(\mathrm{i}\right)$ The  ${\mathrm{E}}_{\mathrm{cell}}^{°}$ of the electrochemical cell representing the reaction is

$2\mathrm{Cr}\left(\mathrm{s}\right)+3{\mathrm{Fe}}^{2+}\left(\mathrm{aq}\right)\to 2{\mathrm{Cr}}^{3+}\left(\mathrm{aq}\right)+3\mathrm{Fe}\left(\mathrm{s}\right)$

$\left(\mathrm{ii}\right)$ The ${\mathrm{E}}_{\mathrm{cell}}$ at  ${25}^{°}\mathrm{C}$ when $\left[{\mathrm{Cr}}^{+3}\right]=0.1 \mathrm{M}$ and $\left[{\mathrm{Fe}}^{2+}\right]=0.01 \mathrm{M}$ will be?

$$\begin{gathered} {\mathrm{E}}_{\raisebox{1ex}{${\mathrm{Cr}}^{+3}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{Cr}$}\right.}^{°}=-0.74\mathrm{\hspace{0.17em}}\mathrm{V} \\ {\mathrm{E}}_{\raisebox{1ex}{${\mathrm{Fe}}^{+2}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{Fe}$}\right.}^{°}=-0.44\mathrm{\hspace{0.17em}}\mathrm{V} \end{gathered}$$

The EMF of a cell corresponding to the reaction:

$\mathrm{Zn}\left(\mathrm{s}\right)+2{\mathrm{H}}^{+}\left(\mathrm{aq}\right)\to {\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right)(0.1\hspace{0.17em}\hspace{0.17em}\mathrm{M})+{\mathrm{H}}_2\left(\mathrm{g}\right)\hspace{0.17em}\hspace{0.17em}(1\hspace{0.17em}\hspace{0.17em}\mathrm{atm}.)\hspace{0.17em}\hspace{0.17em}\mathrm{is}\hspace{0.17em}\hspace{0.17em}0.28\hspace{0.17em}\hspace{0.17em}\mathrm{volt}\hspace{0.17em}\hspace{0.17em}\mathrm{at}\hspace{0.17em}\hspace{0.17em}25°\mathrm{C}.$

The pH of the solution at the hydrogen electrode?
${\text{E}}_{\text{Z}{\text{n}}^{2+}/\text{Z}\text{n}}^{\text{o}}=-0.76\text{v}\text{o}\text{l}\text{t};{\text{E}}_{{\text{H}}^{+}/{\text{H}}_2}^{\text{o}}=0$

If $6.539\times {10}^{-2} \mathrm{g}$ of metallic zinc is added to $100 \mathrm{mL}$ saturated solution of $\mathrm{AgCl}$, then $\mathrm{Ag} \left(\mathrm{s}\right)$ precipitates in the above reaction.

$\left[{\mathrm{K}}_{\mathrm{sp}} \left(\mathrm{AgCl}\right)={10}^{-10}\right]$

(Atomic mass of $\mathrm{Zn}=65.39$)
What is the value of $\log \frac{\left[{\mathrm{Zn}}^{2+}\right]}{{\left[{\mathrm{Ag}}^{+}\right]}^2}$?

$$\begin{gathered} {{\mathrm{E}}^{°}}_{\mathrm{Ag}}=0\mathrm{.}80 \mathrm{V} \\ {{\mathrm{E}}^{°}}_{\mathrm{Zn}}=-0\mathrm{.}76 \mathrm{V} \end{gathered}$$

Find the number of moles of $\mathrm{Ag}$ formed.

A cell, $Ag|A{g}^{+}\parallel C{u}^{2+}|Cu,$ initially contains 1 M $A{g}^{+}$  and 1  $MC{u}^{2+}$ ions.

Calculate the change in the cell potential after the passage of 9.65 A of current for 1 h.

What will be the emf of the given cell  ${\text{Pt | H}}_{\text{2}}{\text{(P}}_{\text{1}}{\text{) | H}}^{\text{+}}{\text{(aq) | H}}_{\text{2}}{\text{(P}}_{\text{2}}\text{) | Pt ?}$

The reduction potential of hydrogen electrode at $25°\mathrm{C}$ in a neutral solution is $\left({\mathrm{P}}_{{\mathrm{H}}_2}=1\text{ atm}\right)$

A hydrogen electrode is made by dipping platinum wire in a solution of nitric acid of $\mathrm{pH}=9$ and passing hydrogen gas around the platinum wire at $1.2$ atm pressure. The oxidation potential of such an electrode equals_______ $\mathrm{V}.$

At $25°\mathrm{C}$, the standard reduction potential for the cell reaction

$\mathrm{Zn}\left(\mathrm{s}\right)+2{\mathrm{H}}^{+}\left(\mathrm{aq}\right)\to {\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right)+{\mathrm{H}}_2( \mathrm{g})$

is $0.28 \mathrm{V}$. What is the reduction potential of the cell reaction in $10 \mathrm{M} \left[{\mathrm{H}}^{+}\right]$ concentration, assuming all other species to be at unit concentration? [Universal gas constant, $\mathrm{R}=8.314 \mathrm{J}{ \mathrm{K}}^{-1}{ \mathrm{mol}}^{-1}$; Faraday constant, $\mathrm{F}=96500{\mathrm{Cmol}}^{-1}]$

In a cell that utilizes the reaction
$\text{Zn(s)}\text{+}{\text{2H}}^{\text{+}}\text{(aq)}\to {\text{Zn}}^{\text{2+}}\text{(aq)}\text{+}{\text{H}}_{\text{2}}\text{(g)}$
addition of H₂SO₄ to cathode compartment,

Which of the following expression(s) represent the voltage of cell at $298 \mathrm{K}?$

$\mathrm{Ag} \left(\mathrm{s}\right)|$$\mathrm{AgI}$ (saturated solution) $\Vert {\mathrm{Ag}}_2{\mathrm{C}}_2{\mathrm{O}}_4$ (saturated solution) $|\mathrm{Ag} (\mathrm{s})$

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 $:\frac{2303\mathrm{RT}}{\mathrm{F}}=0.059$]

What would be the electrode potential for the given half cell reaction at $\mathrm{pH} = 5 ?$

$2{\mathrm{H}}_2\mathrm{O}\to {\mathrm{O}}_2+4{\mathrm{H}}^{\oplus }+4{\mathrm{e}}^{-};{\mathrm{E}}_{\mathrm{red}}^0=1.23 \mathrm{V}$
$\left(\mathrm{R}=8.314 \mathrm{J} {\mathrm{mol}}^{-1} {\mathrm{K}}^{-1};\right.$ temp $=298 \mathrm{K};$ oxygen under std. atm. pressure of $1$ bar)

(Round off answer to the magnitude of nearest integer value)

What is the ${\mathrm{E}}^0$ (in $\mathrm{mV}$) of the reaction when $1 \mathrm{M}$ solution of bismuth trichloride in $1 \mathrm{M} \mathrm{HCl}$ is added to the $1 \mathrm{M}$ solution of tin $\left(\mathrm{II}\right)$ chloride? Use the following data and report answer in '$\mathrm{mV}$'. Assume that the complex formation of the metal ion or its counter ions can't affect the reduction potentials given below.