If the conductivity of mercury at 0$$^\circ$$C is 1.07 $$\times$$ 10⁶ S m^$$-$$1 and the resistance of a cell containing mercury is 0.243$$\Omega$$, then the cell constant of the cell is x $$\times$$ 10⁴ m^$$-$$1. The value of x is ____________. (Nearest integer)

Consider the following cell reaction :

$$C{d_{(s)}} + H{g_2}S{O_{4(s)}} + {9 \over 5}{H_2}{O_{(l)}}$$ $$\rightleftharpoons$$ $$CdS{O_4}.{9 \over 5}{H_2}{O_{(s)}} + 2H{g_{(l)}}$$

The value of $$E_{cell}^0$$ 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 is ___________. (Nearest integer) [Given : Faraday constant = 96487 C mol^$$-$$1]

The resistance of a conductivity cell with cell constant 1.14 cm^$$-$$1, containing 0.001 M KCl at 298 K is 1500 $$\Omega$$. The molar conductivity of 0.001 M KCl solution at 298 K in S cm² mol^$$-$$1 is ____________. (Integer answer)

For the galvanic cell,

Zn(s) + Cu²⁺ (0.02 M) $$\to$$ Zn²⁺ (0.04 M) + Cu(s),

E_cell = ______________ $$\times$$ 10^$$-$$2 V. (Nearest integer)

[Use : $$E_{Cu/C{u^{2 + }}}^0$$ = $$-$$ 0.34 V, $$E_{Zn/Z{n^{2 + }}}^0$$ = + 0.76 V, $${{2.303RT} \over F} = 0.059\,V$$]