In a one-litre flask, 6 moles of A yndergoes the reaction $\mathrm{A}(\mathrm{g}) \rightleftharpoons \mathrm{P}(\mathrm{g})$. The progress of product formation at two temperatures (in Kelvin), $T_1$ and $T_2$, is shown in the figure:
If $T_1=2 T_2$ and $\left(\Delta G_2^{\ominus}-\Delta G_1^{\ominus}\right)=R T_2 \ln x$, then the value of $x$ is $\_\_\_\_$
[ $\Delta \mathrm{G}_1^{\infty}$ and $\Delta \mathrm{G}_2^{\circ}$ are standard Gibb's free energy change for the reaction at temperatures $\mathrm{T}_1$ and $\mathrm{T}_2$, respectively.]
