Applying Raoult's Law to a condensed gas mixture
You have confused the vapor-phase mole fraction with the liquid-phase mole fraction.  The liquid-phase is mole fraction in usually denoted as $x_i$ for compound $i$.  The vapor-phase mole fraction of $i$ is $y_i$.

Raoult's law is that the partial pressure over an ideal solution is equal to the pure-component vapor pressure times the liquid mole fraction, $p_i=x_i*p^°_i$.

Separate from Raoult's law we have the ideal gas law. It says that that says that partial pressures are proportional to mole fraction in the vapor phase, i.e. that $p_i=y_iP$.  So when you took the ratios of $p_{benz}/P$ and $p_{tol}/P$, you were solving for the vapor-phase mole fractions, i.e. for $y_{benz}$ and $y_{tol}$.  

Your mistake comes in taking those $y_i$ values and treating them as $x_i$ values.  That's a mis-formulation of Raoult's law.

You can read more about Raoult's law and the ideal gas law for binary ideal mixtures in my answer to a previous chem.se question.