In a one-litre flask, 6 moles of A undergoes the reaction $\mathrm{A}\left(\mathrm{g}\right)\rightleftharpoons \mathrm{P}\left(\mathrm{g}\right).$  The progress of product formation at two temperatures (in Kelvin), T₁ and  T₂ is shown in the figure:

If ${\mathrm{T}}_1=2{\mathrm{T}}_2\mathrm{and}\left({\mathrm{\Delta G}}_2^{\mathrm{\Theta }}-{\mathrm{\Delta G}}_1^{\mathrm{\Theta }}\right)={\mathrm{RT}}_2\mathrm{lnx},$  then the value of x  is ___.
[${\mathrm{\Delta G}}_1^{\mathrm{\Theta }}\text{and\hspace{0.17em}}{\mathrm{\Delta G}}_2^{\mathrm{\Theta }}$are standard Gibb’s free energy change for the reaction at temperatures  T₁ and T₂  respectively.]