1. Figure 1 gives the experimentally determined phase diagrams for the nearly ideal solution of hexane and heptane. 900 700 500 300 70°C 0.25 0.50 0.75 ZHeptane Figure 1 a) Label the regions of the phase diagram. (c) A liquid mixture is composed of 3 moles of hexane and 2 moles of heptane. If the pressure over the mixture is reduced, estimate the pressure where the first vapor formed.

1. Figure 1 gives the experimentally determined phase diagrams for the nearly ideal solution of hexane and heptane. 900 700 500 300 70°C 0.25 0.50 0.75 ZHeptane Figure 1 a) Label the regions of the phase diagram. (c) A liquid mixture is composed of 3 moles of hexane and 2 moles of heptane. If the pressure over the mixture is reduced, estimate the pressure where the first vapor formed.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Determine the boiling point elevation of a solution of 130.0 mg of carvone (a.k.a. oil of spearmint, C10H14O) dissolved in 1.56 g of carbon disulfide (Kb= 2.34oC/m).
pls answer
A solution containing 0.10 mol of naphthalene (nonvolatile) and 0.90 mol of benzene is cooled until some solid benzene freezes out. The solution is then decanted off from the solid and the decanted solution is warmed to 80°C, at which temperature the vapor pressure above the solution is found to be 670 torr. The normal freezing and boiling points of pure benzene are 5.5 °C and 80°C, respectively and the molar enthalpy of fusion of benzene ∆fus?=10.67 kJ/mol Assume the solution is ideal. a) Calculate the temperature to which the solution was cooled originally. b) Calculate the number of moles of benzene that froze out.
Octane (C8H18) has a vapor pressure of 14.3 torr and a density of 0.703 g/mL. Pentane (CsH12) has a vapor pressure of 435.0 torr and a density of 0.626 g/mL. Assuming a mixture of the two behaved ideally and followed Raoult's Law, what would you predict to be the vapor pressure (in torr) of a solution containing 765 mL of octane and 785 mL of pentane?
A 41.3-gram sample of a solution of naph- thalene, C10H8(s), in benzene, C6H6(l ), has a vapor pressure at 20.0°Cof 63.9 Torr. The vapor pressure of pure benzene at 20.0°C is 75.0 Torr. Assuming that naphthalene has a negligible vapor pressure over the solution, use the vapor pressure–lowering expression to calculate the mole fraction of naphthalene and the number of grams of naphthalene in the solution.
A solution is made by dissolving 0.0475 kg of biphenyl (C₁₂H₁₀) in 350.0 mL of benzene (C₆H₆). If the vapor pressure of pure benzene is 24.4 kPa at 40.0 °C, then what will the vapor pressure of the solution be in kPa? (Consider biphenyl to be nonvolatile and the density of benzene is 0.877 g/mL)
18) A solution is made by dissolving 0.840 moles of sodium hydroxide in 300.0 g of water. If the van't Hoff factor, i, for this particular concentration is 1.70, what is the expected freezing point of this solution? Kf = 1.86 °C m-1. A) +0.80°C B)-2.66°C C) -9.97°C D) -8.85°C E) +3.06°C 18)
List the following aqueous solutions in order of increasing boiling point: 0.120 m glucose, 0.080 m LiBr, 0.050 m Zn(NO3)2, and 0.060 m HF. Assume that the solution is ideal. * glucose < HF < LiBr < Zn(NO3)2 O Zn(NO3)2 < glucose < HF < LIBR O HF < glucose < Zn(NO3)2 < LİBT Zn(NO3)2 < HF < glucose < LiBr
Q5. The depression of the freezing point with FeCl3 s 0.2976 degC and molality is 0.050 m. Calculate the van't Hoff factor i for iron chloride, if the molal freezing depression point constant for water is 1.86 degC/m. Q6.
True or False1.) The phase diagram of a pure solvent shows a lower freezing point compared to solutions2.) The process of freezing only lowers the kinetic energy of solute particles in a solution3.) Ionic solutes have higher van't hoff factor compared to non ionic solutes4.) The formation of intermolecular forces of attraction requires complete dissolution
Do not give handwriting solution.
A 1.00 molal aqueous solution of trichloroacetic acid (CCl3COOH) is heated to its boiling point. The solution has the boiling point of 100.18°C. Determine the van’t Hoff factor for trichloroacetic acid. (Kb for water = 0.512 K kg mol-1)