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Biphenyl, C12H10, is a nonvolatile, nonionizing solute that is soluble in benzene, C6H6. At 25 °C,...

Biphenyl, C12H10, is a nonvolatile, nonionizing solute that is soluble in benzene, C6H6. At 25 °C, the vapor pressure of pure benzene is 100.84 torr. What is the vapor pressure of a solution made from dissolving 11.8 g of biphenyl in 33.3 g of benzene?

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Expert Solution

no of moles of Biphenyl nC12H10   = W/G.M.Wt

                                                         = 11.8/154 = 0.076moles

no of moles of Benzene n C6H6    = W/G.M.Wt

                                                         = 33.3/78   = 0.427 moles

mole fraction of Benzene XC12H10   = nC6H6/nC12H10 + nC6H6

                                                           = 0.427/0.427+0.076

                                                            = 0.427/0.503   = 0.849

The vapor pressure of pure benzene = 100.84 torr

the vapore pressure of solution = P = P^0XC6H6

                                                           = 100.84*0.849   = 85.6 torr

queen_honey_blossom answered 2 years ago
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