Exercise-4

The electrode potentials for ${\mathrm{Cu}}^{2+}\left(\mathrm{aqueous}\right)+{\mathrm{e}}^{-}⟶{\mathrm{Cu}}^{+}\left(\mathrm{aqueous}\right)$ and ${\mathrm{Cu}}^{+} \left(\mathrm{aqueous}\right)+{\mathrm{e}}^{-}⟶\mathrm{Cu} \left(\mathrm{s}\right)$ are $+0.15 \mathrm{V}$ and $+0.50 \mathrm{V},$ respectively. The value of $\mathrm{E}{°}_{{\mathrm{Cu}}^{2+}/\mathrm{Cu}}$ will be:

The specific conductance of $\mathrm{a}=1 \mathrm{M} \mathrm{KCl}$ solution at $23°\mathrm{C}$ is $0.012{\mathrm{ohm}}^{-1}{ \mathrm{cm}}^{-1}.$ The resistance of the cell containing the solution at the same temperature was found to be $55 \mathrm{ohm}.$ The cell constant will be

When a metal is electroplated with silver $\left(\mathrm{Ag}\right)$ 

The best reducing agent among the following is:

$\mathrm{E}$ of the given cell is:

$\mathrm{Ni}\left|({\mathrm{Ni}}^{+2},1.0\mathrm{M})\Vert \left({\mathrm{Co}}^{+2},1.0\mathrm{M}\right)\right|\mathrm{Co}$

From the given standard electrode potentials,
${\mathrm{Sn}}^{4+}\left(\mathrm{aq}\right)+2{\mathrm{e}}^{-}\to {\mathrm{Sn}}^{2+}\left(\mathrm{aq}\right) \mathrm{E}°=0.15 \mathrm{V}$

${\mathrm{Br}}_2\left(\mathrm{l}\right)+2{\mathrm{e}}^{-}\to 2{\mathrm{Br}}^{-}\left(\mathrm{aq}\right) \mathrm{E}°=1.07 \mathrm{V}$

The approximate free energy change of the process $2{\mathrm{Br}}^{-}\left(\mathrm{aq}\right)+{\mathrm{Sn}}^{4+}\left(\mathrm{aq}\right)\to {\mathrm{Br}}_2\left(\mathrm{l}\right)+{\mathrm{Sn}}^{2+}\left(\mathrm{aq}\right)$ is

The standard electrode potential $\left({\mathrm{E}}^{\mathrm{o}}\right)$ of the Daniel cell is $1.1 \mathrm{V}$ $\mathrm{Zn}\left(\mathrm{s}\right)+{\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right)⟶{\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right)+\mathrm{Cu}\left(\mathrm{s}\right).$ Under which of the following conditions will the cell potential be higher than $1.1 \mathrm{V}$?

The metal that cannot be displaced from its aqueous solution by zinc is.