At $298 \mathrm{K}$, the conductivity of pure water is $5.5\times {10}^{-6} {\mathrm{Sm}}^{-1}$. Calculate the ionic product of water using the following data:
${\mathrm{\lambda }}_{\mathrm{m}}^{\mathrm{o}}$ values $\left(\mathrm{in} \mathrm{S} {\mathrm{m}}^2 {\mathrm{mol}}^{-1}\right): \mathrm{Ba}(\mathrm{OH}{)}_2=5.3\times {10}^{-2}, \mathrm{HCl}=4.25\times {10}^{-2}, {\mathrm{BaCl}}_2=2.8\times {10}^{-2}$
Does your answer match with experimental value. Write $20$ for yes &$40$ for No.

Given ${{\mathrm{E}}^{\mathrm{o}}}_{{\mathrm{Ag}}^{+}/\mathrm{Ag}}=0.80 \mathrm{V}, {{\mathrm{E}}^{\mathrm{o}}}_{{\mathrm{Mg}}^{2+}/\mathrm{Mg}}=-2.37 \mathrm{V}, {{\mathrm{E}}^{\mathrm{o}}}_{{\mathrm{Cu}}^{2+}/\mathrm{Cu}}=0.34 \mathrm{V}, {{\mathrm{E}}^{\mathrm{o}}}_{{\mathrm{Hg}}^{2+}/\mathrm{Hg}}=0.79 \mathrm{V}$.

Which of the following statements is/are correct.

The resistances of following solutions of $\mathrm{KCl}$ were measured using conductivity cells of different cell constants, at same temperature. (Consider that at concentration less than $0.1 \mathrm{M}$ , the specific conductivity of solution is directly proportional to the concentration of solution.) 

$\begin{array}{|lll|}\hline & \text{ Concentration of Solution }& \text{ Cell Constant }\\ 1.& 0.1\mathrm{M}& 1{\mathrm{cm}}^{-1}\\ 2.& 0.01\mathrm{M}& 10{\mathrm{cm}}^{-1}\\ 3.& 0.005\mathrm{M}& 5{\mathrm{cm}}^{-1}\\ 4.& 0.0025\mathrm{M}& 25{\mathrm{cm}}^{-1}\\ \hline\end{array}$

Which of the following comparisons between their conductances $\left(\mathrm{G}\right)$ is/are correct?