At $310 \mathrm{K}$, the solubility of ${\mathrm{CaF}}_2$ in water is $2.34\times {10}^{-3} \mathrm{g}/100 \mathrm{mL}$. The solubility product of ${\mathrm{CaF}}_2$ is ---- $\times {10}^{-8}{\left(\mathrm{mol}/\mathrm{L}\right)}^3$(nearest integer). (Given molar mass : ${\mathrm{CaF}}_2=78 \mathrm{g}{ \mathrm{mol}}^{-1}$)

At $600 \mathrm{K},2 \mathrm{mol}$ of $\mathrm{NO}$ are mixed with $1 \mathrm{mol}$ of ${\mathrm{O}}_2$.

$2{\mathrm{NO}}_{\left(\mathrm{g}\right)}+{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftarrows 2{\mathrm{NO}}_2\left(\mathrm{g}\right)$

The reaction occurring as above comes to equilibrium under a total pressure of $1$ atm. Analysis of the system shows that $0.6 \mathrm{mol}$ of oxygen are present at equilibrium. The equilibrium constant ${\mathrm{K}}_{\mathrm{p}}$ for the reaction is____. Give an answer to the nearest integer value.

Consider the following reaction approaching equilibrium at $27°\mathrm{C}$ and $1$ atm pressure

$\mathrm{A}+\mathrm{B}\underset{{\mathrm{K}}_{\mathrm{r}}={10}^2}{\stackrel{{\mathrm{K}}_{\mathrm{t}}=0^3}{\rightleftharpoons }}\mathrm{C}+\mathrm{D}$

The standard Gibb's energy change $\left({\mathrm{\Delta }}_{\mathrm{r}}\mathrm{G}°\right)$ at $27°\mathrm{C}$ is $\left(-\right)$ _____ ${\mathrm{kJmol}}^{-1}$ (Nearest integer).

(Given : $\mathrm{R}=8.3\mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1}$ and $\ln 10=2.3$)