Ask Question
31 March, 18:31

At a given temperature, you have a mixture of benzene (vapor pressure of pure benzene = 745 torr) and toluene (vapor pressure of pure toluene = 290 torr). The mole fraction of benzene in the vapor above the solution is 0.590. Assuming ideal behavior, calculate the mole fraction of toluene in the solution.

+2
Answers (1)
  1. 31 March, 18:32
    0
    Ideal solutions obey Raoult's law, which states that:

    P_i = x_i * (P_pure) _i

    where

    P_i is the partial pressure of component i above a solution

    x_i is the mole fraction of component i in the solution

    (P_pure) _i is the vapor pressure of pure component i

    In this case,

    P_benzene = 0.59 * 745 torr = 439.6 torr

    P_toluene = (1-0.59) * 290 torr = 118.9 torr

    The total vapor pressure above the solution is the sum of the vapor pressures of the individual components:

    P_total = (439.6 + 118.9) torr = 558.5 torr

    Assuming the gas phase also behaves ideally, the partial pressure of each gas in the vapor phase is proportional to its molar concentration, so the mole fraction of toluene in the vapor phase is:

    118.9 torr/558.5 torr = 0.213
Know the Answer?
Not Sure About the Answer?
Find an answer to your question 👍 “At a given temperature, you have a mixture of benzene (vapor pressure of pure benzene = 745 torr) and toluene (vapor pressure of pure ...” in 📗 Chemistry if the answers seem to be not correct or there’s no answer. Try a smart search to find answers to similar questions.
Search for Other Answers