Benzene,C₆H₆,and toluene,C₆H₅CH₃,form ideal solutions.At 35°C the vapor pressure of benzene is 160.torr and that of toluene is 50.0 torr.In an experiment,55.6 g of benzene and 86.6 g of toluene are placed in a closed container at 35°C.At equilibrium,what is the partial vapor pressure of toluene? A)103 torr B)91.634 torr C)21.5 torr D)68.9 torr E)28.4 torr

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Quizplus · Accepted Answer

To find the partial vapor pressure of toluene in the solution, we use Raoult's law, which states that the partial vapor pressure of a component in a solution is equal to the vapor pressure of the pure component multiplied by its mole fraction in the solution. First, calculate the moles of benzene and toluene using their molar masses (benzene = 78.11 g/mol, toluene = 92.14 g/mol). Moles of benzene = 55.6 g / 78.11 g/mol = 0.7118 mol. Moles of toluene = 86.6 g / 92.14 g/mol = 0.9402 mol. Total moles = 0.7118 mol + 0.9402 mol = 1.652 mol. Mole fraction of toluene = 0.9402 mol / 1.652 mol = 0.569. Partial vapor pressure of toluene = 0.569 * 50.0 torr = 28.4 torr.

Benzene,C6H6,and Toluene,C6H5CH3,form Ideal Solutions

Benzene,C₆H₆,and Toluene,C₆H₅CH₃,form Ideal Solutions