An electrochemical cell can behave like an electrolytic cell when . . . . . . .

In the process of obtaining chlorine from brine,the minimum value of $E_{cell}$ should be ....... $V$.

Match List – $I$ (Laws) with the List – $II$ (Mathematical expression):

List – $I$	List – $II$
$(a)$ Henry’s law	$(i)$ $p_1 = x_1 p_1^o$
$(b)$ Raoult’s law	(ii) $p = K_H x$
$(c)$ First law of thermodynamics	(iii) $\Lambda_m^o = \nu_+ \lambda_+^o + \nu_- \lambda_-^o$
$(d)$ Kohlrausch’s law	(iv) $\Delta U = q + w$

The equilibrium constant for the reaction $Zn_{(s)} + Sn^{2+}_{(aq)} \rightleftharpoons Zn^{2+}_{(aq)} + Sn_{(s)}$ is $1 \times 10^{20}$ at $298 \ K$. The magnitude of standard electrode potential of $Sn/Sn^{2+}$ if $E_{Zn^{2+}/Zn}^0 = -0.76 \ V$ is $............ \times 10^{-2} \ V$. (Nearest integer)
Given : $\frac{2.303 \ RT}{F} = 0.059 \ V$

$A$ fuel cell uses $CH_4$ gas and it forms $CO_3^{2-}$ at the anode. It is used to power a car with $96.5 \ A$ for $10000 \ s$. The volume of $CH_4$ gas required at $1 \ atm$ and $273 \ K$ is $............ \ L$.

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?