The standard cell voltage for the cell $\mathrm{Pb}\left|{\mathrm{Pb}}^{2+}\right|\left|{\mathrm{Sn}}^{2+}\right|\mathrm{Sn}$ is $-0.01\text{V}.$
If the cell is to exhibit ${\mathrm{E}}_{\mathrm{cell}}=0$, the value of $\frac{\left[{\mathrm{Sn}}^{2+}\right]}{\left[{\mathrm{Pb}}^{2+}\right]}$ should be antilog of

Calculate ${\mathrm{\Lambda }}^{\circ }$ $\left(\mathrm{HOAc}\right)$ using appropriate molar conductance of the electrolytes listed above at infinite dilution in the water at $25°\mathrm{C}$.

The equivalent conductance of two strong electrolytes at infinite dilution in ${\mathrm{H}}_2\mathrm{O}$ (where ions move freely through a solution) at $25°\mathrm{C}$ are given below:

${\mathrm{\Lambda }}^{\circ }\left({\mathrm{CH}}_3\mathrm{COONa}\right)=91.0 \mathrm{S} {\mathrm{cm}}^2/\mathrm{equivalent}$

${\mathrm{\Lambda }}^{\circ }\left(\mathrm{HCl}\right)=426.2 \mathrm{S} {\mathrm{cm}}^2/\mathrm{equivalent}$

What additional information/quantity does one need to calculate ${\mathrm{\Lambda }}^{\circ }$ of an aqueous solution of acetic acid?

Two lead storage batteries were operated in separate experiments (I, II).

I. The maximum work obtained was '$\mathrm{X}$' at cell potential $2 \mathrm{V}$ consuming $1$ mole of lead.
II. The maximum work obtained was '$\mathrm{Y}$' at cell potential $1.5 \mathrm{V}$ consuming $0.1$ mole of lead.

Then, $\mathrm{X}:\mathrm{Y}$ is: