Consider a solvent whose molecular weight is 200.0 amu and whose vapor pressure at 25 ºC is 35.00 mm Hg. A sample of 100.0 g of a solute whose molecular weight is 100.00 amu is dissolved in 1.000 kg of that solvent. The solute is not an electrolyte. The vapor pressure of the pure solute is 0.01 mm Hg at 25 ºC. What is the vapor pressure of the solution at 25 ºC?

Hi i was wondering if anyone knows where i can start. Someone told me to use Molar Fractions but this problem is confusing. i dont really understand whats goin on. might also be related to Raoult's law: Pa=XaP'a, Pa=Vapor Pressure of the solution Xa=Mole Fraction of solvent P'a=Vapor Presure of pure solvent. but how would i use it?.. they give Vapor pressure of the pure solvent. but i dunno how to compile the other information nor do i know what they mean...any help is appreciated

How do u calculate the moles of an unknown substance, with grams. and am i suppose to 1amu=1.66054E-24g?

ok nvm someone helped me get the solution. if anyone wanted to know its.. Psol'n = 35 mm Hg x (1000g/200) / ( 1000/200 + 100/100)