Berthelot proposed the following empirical relation to explain the real behaviour of the real gases :

$\left(\mathrm{P}+\frac{\mathrm{a}}{{\mathrm{TV}}^2}\right)(\mathrm{V}-\mathrm{b})=\mathrm{RT}$

If the Berthelot equation of state be one of the forms of virial equation for 1 mole real gas is as under:

$\mathrm{PV}=\mathrm{RT}\left[1+\frac{\mathrm{A}}{\mathrm{V}}+\frac{\mathrm{B}}{{\mathrm{V}}^2}+\frac{\mathrm{C}}{{\mathrm{V}}^3}+\dots . \mathrm{to} \mathrm{higher} \mathrm{powe} \mathrm{rof} \mathrm{n}\right]$

where A, B and C are constants which are known as second, third and fourth virial coefficients respectively. Then what will be the correct value of Boyle's temperature i.e., ${\mathrm{T}}_{\mathrm{B}}$ i.e., the temperature at which $\mathrm{PV}=\mathrm{RT}$ i.e., ideal gas equation is obeyed?