At 300°K, the vapor pressure of pure benzene (C6H6) is 0.1355 atm and the vapor pressure of pure n-hexane (C6H14) is 0.2128 atm. Mixing 50.0 g benzene with 50.0 g of n-hexane gives a solution that is nearly ideal. a. Calculate the mole fraction of benzene in the solution. b. Calculate the total vapor pressure of the solution at 300 K.
At 300°K, the vapor pressure of pure benzene (C6H6) is 0.1355 atm and the vapor pressure of pure n-hexane (C6H14) is 0.2128 atm. Mixing 50.0 g benzene with 50.0 g of n-hexane gives a solution that is nearly ideal.
a. Calculate the mole fraction of benzene in the solution.
b. Calculate the total vapor pressure of the solution at 300 K.
c. Calculate the mole fraction of benzene in the vapor in equilibrium with the solution.
d. Compare the mole fraction of benzene in the solution with the mole fraction of benzene in the vapor. Explain your observation.
e. If this vapor were collected and then recondensed, what would the mole fraction of benzene in this new solution be?
f. If the new solution were allowed to come to equilibrium, what would the mole fraction of benzene in the vapor in equilibrium with the solution be?
g. Predict what would happen if this were done many times. How could this be useful in chemical experiments?
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