The number of moles of ${\mathrm{NH}}_3,$ that must be added to $2 \mathrm{L}$ of $0.80{\mathrm{MAgNO}}_3$ in order to reduce the concentration of ${\mathrm{Ag}}^{+}$ ions to $5.0\times {10}^{-8}\mathrm{M}\left({\mathrm{K}}_{\text{formation }}\right.$ for $\left.{\left[\mathrm{Ag}{\left({\mathrm{NH}}_3\right)}_2\right]}^{+}=1.0\times {10}^8\right)$ is __________. (Nearest integer)
[Assume no volume change on adding ${\mathrm{NH}}_3$]

For the reaction

$\mathrm{A}+\mathrm{B}\rightleftharpoons 2\mathrm{C}$

the value of equilibrium constant is $100$ at $298 \mathrm{K}$. If the initial concentration of all the three species is $1 \mathrm{M}$ each, then the equilibrium concentration of $\mathrm{C}$ is $\mathrm{x}\times {10}^{-1} \mathrm{M}$. The value of $\mathrm{x}$ is _______. (Nearest integer)