For the reaction A ( g ) ⇌ B ( g ) at 495 K, Δ_r G^°=-9.478 kJ mol^-1. If we start the reaction in a closed container at 495 K with 22 millimoles of…

For the reaction $\displaystyle \mathrm{A}(\mathrm{g}) \rightleftharpoons \mathrm{B}(\mathrm{g})$ at $\displaystyle 495 \mathrm{~K}, \Delta_{\mathrm{r}} \mathrm{G}^{\circ}=-9.478 \mathrm{~kJ} \mathrm{~mol}^{-1}$. If we start the reaction in a closed container at $\displaystyle 495$ K with $\displaystyle 22$ millimoles of A, the amount of B in the equilibrium mixture is \_\_\_\_ millimoles. (Round off to the Nearest Integer). $\displaystyle \left[\mathrm{R}=8.314 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1} ; \ln 10=2.303\right]$