The solubility of ${\mathrm{BaSO}}_4$ in pure water (in $\mathrm{g} {\mathrm{L}}^{-1}$) is the closest to [Given: ${\mathrm{K}}_{\mathrm{sp}}$ for ${\mathrm{BaSO}}_4$ is $1.0\times {10}^{-10}$ at $25°\mathrm{C}$. Molecular weight of ${\mathrm{BaSO}}_4$ is $233 \mathrm{g} {\mathrm{mol}}^{-1}$]

From equations $1$ and $2$,

${\mathrm{CO}}_2\rightleftharpoons \mathrm{CO}+\frac{1}{2}{\mathrm{O}}_2$ $[{\mathrm{K}}_{{\mathrm{c}}_1}=9.1\times {10}^{-12}$ at $1000°\mathrm{C}]$ (equation $1$)

${\mathrm{H}}_2\mathrm{O}\rightleftharpoons {\mathrm{H}}_2+\frac{1}{2}{\mathrm{O}}_2$ $[{\mathrm{K}}_{{\mathrm{c}}_2}=7.1\times {10}^{-12}$ at $1000°\mathrm{C}]$ (equation $2$)

find out ${\mathrm{K}}_{\mathrm{c}}$ ,for the following equation ${\mathrm{CO}}_2+{\mathrm{H}}_2\rightleftharpoons \mathrm{CO}+{\mathrm{H}}_2\mathrm{O}$.

The equilibrium constant for the following reactions are ${\mathrm{K}}_1$ and ${\mathrm{K}}_2$, respectively.

$2{\mathrm{P}}_{\left(\mathrm{g}\right)}+3{{\mathrm{Cl}}_2}_{\left(\mathrm{g}\right)}\rightleftharpoons 2{{\mathrm{PCl}}_3}_{\left(\mathrm{g}\right)}$

${{\mathrm{PCl}}_3}_{\left(\mathrm{g}\right)}+{{\mathrm{Cl}}_2}_{\left(\mathrm{g}\right)}\rightleftharpoons {{\mathrm{PCl}}_5}_{\left(\mathrm{g}\right)}$

The equilibrium constant for the reaction $2{\mathrm{P}}_{\left(\mathrm{g}\right)}+5{{\mathrm{Cl}}_2}_{\left(\mathrm{g}\right)}\rightleftharpoons 2{{\mathrm{PCl}}_5}_{\left(\mathrm{g}\right)}$: