Find the solubility product $(K_{sp})$ of a saturated solution of $Ag_2CrO_4$ in water at $298 \ K$,if the $emf$ of the cell $Ag | Ag^{+} (\text{satd. } Ag_2CrO_4 \text{ solution}) || Ag^{+} (0.1 \ M) | Ag$ is $0.591 \ V$ at $298 \ K$.

$A$ hydrogen electrode is immersed in a solution with $pH = 0$ $(HCl)$. By how much will the potential (reduction) change if an equivalent amount of $NaOH$ is added to the solution? (Take $pH_2 = 1 \ atm$,$T = 298 \ K$).

$A$ battery is made from $Cr$ and $Na_2Cr_2O_7$. When this battery discharges according to the reaction $Na_2Cr_2O_7 + Cr + H^{+} \rightarrow Cr^{3+} + H_2O + Na^{+}$,the chemical equation is unbalanced. If $1 \ F$ (Faraday) of electricity is passed during the charging of the battery,what is the number of moles of $Cr^{3+}$ removed from the solution (in $/3$)?

$Cu^{+}$ ion is not stable in aqueous solution because of disproportionation reaction. $E^o$ value for disproportionation of $Cu^{+}$ is .............. $V$ (Given $E^o_{Cu^{2+}/Cu^{+}} = 0.15 \ V$,$E^o_{Cu^{2+}/Cu} = 0.34 \ V$)

If $63.5 \ g$ of $Cu$ is deposited on the electrode from a $CuSO_4$ solution,what is the number of electrons involved?

Consider the following cell reaction:
$Cd_{(s)} + Hg_{2}SO_{4(s)} + \frac{9}{5}H_{2}O_{(l)} \rightleftharpoons CdSO_{4} \cdot \frac{9}{5}H_{2}O_{(s)} + 2Hg_{(l)}$
The value of $E_{\text{cell}}^{0}$ is $4.315 \ V$ at $25^{\circ}C$. If $\Delta H^{\circ} = -825.2 \ kJ \ mol^{-1}$,the standard entropy change $\Delta S^{\circ}$ in $J \ K^{-1} \ mol^{-1}$ is ........ . (Nearest integer) [Given: Faraday constant $= 96487 \ C \ mol^{-1}$]