Select the incorrect option,when a lead storage battery is discharged $-$

Which one of the following is the correct plot of $\Lambda_m$ (in $S \ cm^2 \ mol^{-1}$) and $\sqrt{C}$ (in $mol^{1/2} \ L^{-1/2}$) for a $KCl$ solution? ($y=\Lambda_m$; $x=\sqrt{C}$)

When does the galvanic cell become an electrolytic cell?

The value of the standard electrode potential for the oxidation of $Cl^{-}$ ions is more positive than that of water. Even then,in the electrolysis of aqueous sodium chloride,why is $Cl^{-}$ oxidized at the anode instead of water?

The standard reduction potential data at $25^{\circ} C$ is given below.
$E^{\circ}(Fe^{3+}, Fe^{2+}) = +0.77 \ V$
$E^{\circ}(Fe^{2+}, Fe) = -0.44 \ V$
$E^{\circ}(Cu^{2+}, Cu) = +0.34 \ V$
$E^{\circ}(Cu^{+}, Cu) = +0.52 \ V$
$E^{\circ}(O_{2(g)} + 4H^{+} + 4e^{-} \rightarrow 2H_{2}O) = +1.23 \ V$
$E^{\circ}(O_{2(g)} + 2H_{2}O + 4e^{-} \rightarrow 4OH^{-}) = +0.40 \ V$
$E^{\circ}(Cr^{3+}, Cr) = -0.74 \ V$
$E^{\circ}(Cr^{2+}, Cr) = -0.91 \ V$
Match $E^{\circ}$ of the redox pair in List-$I$ with the values given in List-$II$ and select the correct answer using the code given below the lists:

List-$I$	List-$II$
$P. \ E^{\circ}(Fe^{3+}, Fe)$	$1. \ -0.18 \ V$
$Q. \ E^{\circ}(4H_{2}O \rightleftharpoons 4H^{+} + 4OH^{-})$	$2. \ -0.4 \ V$
$R. \ E^{\circ}(Cu^{2+} + Cu \rightarrow 2Cu^{+})$	$3. \ -0.04 \ V$
$S. \ E^{\circ}(Cr^{3+}, Cr^{2+})$	$4. \ -0.83 \ V$

Codes: $P \quad Q \quad R \quad S$

Explain the redox reaction of electrodes with the example of a Daniell cell.