Raoult's Law confusion
It should be like:

The saturated partial pressure of each component of an ideal mixture of liquids is equal to the saturated vapour pressure of the pure component multiplied by its mole fraction in the liquid mixture.

These data are independent on the actual composition of the gaseous phase, that may, or may not be in the equilibrium with the liquid.
OTOH, composition of the liquid phase does depend on the amount and composition of the original liquid mixture put into a container, as evaporation changes liquid composition in favour of less volatile component.
If the pure liquid $\mathrm{A}$ has saturated vapour presure $p_\mathrm{0,A}$
and the pure liquid $\mathrm{B}$ has saturated vapour presure $p_\mathrm{0,B}$
and if the $\mathrm{A}$ in the liquid has molar fraction $x_\mathrm{A,l}$,
then the gaseous molar fraction of $\mathrm{A}$ ( in the saturated gaseous phase, with assumption of ideal behaviour given by the Raoult law ) is:
$$x_\mathrm{A,g} = \frac{x_\mathrm{A,l} \cdot p_\mathrm{0,A}}{ x_\mathrm{A,l} \cdot p_\mathrm{0,A} + (1-x_\mathrm{A,l}) \cdot p_\mathrm{0,B}}$$
For calculation for particular volumes of the container and the initial mixture of volumes, you would need more data, like these volumes and densities, and assumptions how to treat gases, like. e.g. as the ideal gas, but it goes behind the Raoult law. In all the complexity, it is solving a set of equations for set of variables, like molar amounts in both phases and phase volumes.
If the fraction of components in the gaseous volume is negligible, e.g. if we consider the total vapour pressure in a full or almost full container, we can consider total mixture composition is the same as liquid composition.