11.37. A solution contains 3.5 moles of water and 1.5 moles
of nonvolatile glucose ($C_6H_{12}O_6$). What is the mole
fraction of water in this solution? What is the vapor
pressure of the solution at 25°C, given that the vapor
pressure of pure water at 25°C is 23.8 torr?
11.38. A solution contains 4.5 moles of water, 0.3 moles of
sucrose ($C_{12}H_{22}O_{11}$), and 0.2 moles of glucose.
Sucrose and glucose are nonvolatile. What is the
mole fraction of water in this solution? What is the
vapor pressure of the solution at 35°C, given that the
vapor pressure of pure water at 35°C is 42.2 torr?
11.39. Another way of stating Raoult's law is that the
fractional lowering of the vapor pressure of the
solvent in a solution ($P_{solvent}^o - P_{solvent}$)/$P_{solvent}^o$ is
equal to the mole fraction of the solute, $X_{solute}$. Use
Equation 11.7 to show that this is true.
11.40. Use the statement of Raoult's law in Problem 11.39
to determine the mole fraction of glucose in
Problem 11.37.
