16. (Ch6) At 25^circ C the vapor pressure of pure benzene (C_(6)H_(6)) is 0.1252 atm. How many moles of any nonvolatile, nondissoci ating solute must be added to 156 g of pure benzene at 25^circ C to result in a solution vapor pressure of 0.1000 atm ? a. 0.252 b. 0.337 c. 0.504 d. 0.674 e. 0.8

To solve this problem, we can use Raoult's Law, which states that the vapor pressure of a solvent in a solution is directly proportional to the mole fraction of the solvent in the solution. The formula for Raoult's Law is: where:- is the vapor pressure of the solution,- is the mole fraction of the solvent in the solution,- is the vapor pressure of the pure solvent.Given:- (vapor pressure of pure benzene) = 0.1252 atm- (vapor pressure of the solution) = 0.1000 atm- Mass of benzene = 156 gFirst, we need to find the number of moles of benzene. The molar mass of benzene ( ) is approximately 78.11 g/mol. Next, we use Raoult's Law to find the mole fraction of benzene in the solution: Let be the moles of the solute added. The total moles in the solution will be: The mole fraction of benzene is then: Solving for : Therefore, the number of moles of the solute needed is approximately 0.513 moles. The closest answer to this is:c. 0.504