Impure copper containing $Fe$,$Au$,and $Ag$ as impurities is electrolytically refined. $A$ current of $140 \ A$ for $482.5 \ s$ decreased the mass of the anode by $22.26 \ g$ and increased the mass of the cathode by $22.011 \ g$. The percentage of iron in the impure copper is (Given molar mass $Fe = 55.5 \ g \ mol^{-1}$,molar mass $Cu = 63.54 \ g \ mol^{-1}$)

On the basis of standard electrode potential values,suggest which of the following reactions would take place?

Match the entries from Column $I$ and Column $II$ and choose the correct order.

$A$. Leclanche cell	$1$. Converts energy of combustion into electrical energy
$B$. Fuel cell	$2$. Rechargeable cell
$C$. Ni-Cd cell	$3$. At anode,$Zn \longrightarrow Zn^{2+} + 2e^{-}$

Which of the following statements is incorrect?

The standard electrode potential $E^{\ominus}$ and its temperature coefficient $\left( \frac{dE^{\ominus}}{dT} \right)$ for a cell are $2 \ V$ and $-5 \times 10^{-4} \ V \ K^{-1}$ at $300 \ K$ respectively. The cell reaction is
$Zn_{(s)} + Cu^{2+}_{(aq)} \rightleftharpoons Zn^{2+}_{(aq)} + Cu_{(s)}$
Standard reaction enthalpy $\left( \Delta_r H^{\ominus} \right)$ is ....... $kJ$

The number of incorrect statements from the following is:
$A.$ The electrical work that a reaction can perform at constant pressure and temperature is equal to the reaction Gibbs energy.
$B.$ $E_{cell}^0$ is dependent on the pressure.
$C.$ $\frac{dE_{cell}^0}{dT} = \frac{\Delta_{r}S^0}{nF}$.
$D.$ $A$ cell is operating reversibly if the cell potential is exactly balanced by an opposing source of potential difference.