$1\times {10}^{-5} \mathrm{M} {\mathrm{AgNO}}_3$ is added to $1 \mathrm{L}$ of saturated solution of $\mathrm{AgBr}$. The conductivity of this solution at $298 \mathrm{K}$ is $\_\_\_\_\_\_\_\times {10}^{-8} \mathrm{S} {\mathrm{m}}^{-1}$.

[Given : ${\mathrm{K}}_{\mathrm{sp}}\left(\mathrm{AgBr}\right)=4.9\times {10}^{-13}$ at $298 \mathrm{K}$

${\lambda }_{{\mathrm{Ag}}^{+}}^0=6\times {10}^{-3}{\mathrm{Sm}}^2 {\mathrm{mol}}^{-1}$

${\lambda }_{{\mathrm{Br}}^{-}}^0=8\times {10}^{-3}{\mathrm{Sm}}^2 {\mathrm{mol}}^{-1}$

$\left.{\lambda }_{{\mathrm{NO}}_3^{-}}^0=7\times {10}^{-3}{\mathrm{Sm}}^2 {\mathrm{mol}}^{-1}\right]$

For the reaction
$2{\mathrm{Fe}}^{3+}\left(\mathrm{aq}\right)+2{\mathrm{I}}^{-}\left(\mathrm{aq}\right)\to 2{\mathrm{Fe}}^{2+}\left(\mathrm{aq}\right)+{\mathrm{I}}_2( \mathrm{s})$
the magnitude of the standard molar free energy change, ${∆}_{\mathrm{r}}{\mathrm{G}}_{\mathrm{m}}^{\circ }=-$______$\mathrm{kJ}$ (Round off to the Nearest Integer).

A $5.0 \mathrm{m} \mathrm{mol} {\mathrm{dm}}^{-3}$ aqueous solution of $\mathrm{KCl}$ has a conductance of $0.55 \mathrm{mS}$ when measured in a cell constant $1.3{ \mathrm{cm}}^{-1}$. The molar conductivity of this solution is _______ ${\mathrm{mSm}}^2{ \mathrm{mol}}^{-1}$. (Round off to the Nearest Integer)