The electrolyte used in a mercury cell is:

Given $\lambda^{\circ}_{Mg^{2+}} = 106 \ S \ cm^2 \ mole^{-1}$ and $\lambda^{\circ}_{SO_4^{2-}} = 160 \ S \ cm^2 \ mole^{-1}$. The value of $\lambda^{\circ}_{MgSO_4}$ (in $S \ cm^2 \ mole^{-1}$) is

Assertion : Galvanised iron does not rust.
Reason : Zinc has a more negative electrode potential than iron.

$E^{\circ}_{Cu^{2+}|Cu} = +0.34 \ V$
$E^{\circ}_{Zn^{2+}|Zn} = -0.76 \ V$
Identify the incorrect statement from the options below for the above 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?

For a $Ag-Zn$ button cell,the net reaction is $Zn_{(s)} + Ag_{2}O_{(s)} \rightarrow ZnO_{(s)} + 2Ag_{(s)}$. Given $\Delta G_{f}^{o}(Ag_{2}O) = -11.21 \ kJ \ mol^{-1}$ and $\Delta G_{f}^{o}(ZnO) = -318.3 \ kJ \ mol^{-1}$,the $E^{o}_{cell}$ of the button cell is ......... $V$.