13.10 This portion of a phase diagram shows the vapor-pressure curves of a volatile solvent and of a solution of that solvent containing a nonvolatile solute. (a) Which line represents the solution? (b) What are the normal boiling points of the solvent and the solution? [Section 13.5] Com Centra 1.0 3 40 50 70 60 TОC) P (atm)

13.10 This portion of a phase diagram shows the vapor-pressure curves of a volatile solvent and of a solution of that solvent containing a nonvolatile solute. (a) Which line represents the solution? (b) What are the normal boiling points of the solvent and the solution? [Section 13.5] Com Centra 1.0 3 40 50 70 60 TОC) P (atm)

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...

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10:16 S 57% Question 11 of 15 0/2 POINTS EARNED A solution made by dissolving 150.0 g of an unknown compound in 425.0 mL of 12 benzene to make a solution which has a freezing point 18.6 °C lower than that of pure benzene. Kf for benzene is 5.12 °C/m and the density of benzene is 0.877 g/mL. What was the molality of the solution? a O of 0.67 points earned L 3 attempts remaining How many moles of the unknown compound were dissolved in the b solution? L 0 of 0.67 points earned 3 attempts remaining What is the molar mass of the unknown compound? L O of 0.67 points earned 3 attempts remaining II
An aqueous solution contains the amino acid glycine (NH2CH2COOH). Assuming that the acid does not ionize in water, calculate the molality, in molal, of the solution if it freezes at - 2.83 °C. (Cryoscopic constant of water: 1.86 °C/molal; Atomic Weight: N = 14.01 g/mol; H = 1.008 g/mol; C = 12.01 g/mol; O = 16.00 g/mol; density of water = 1.00 g/mL). Express your answer in three %3D decimal places only. Do not put the units.
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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.
Glycerin (C3H8O3) is a nonvolatile nonelectrolyte. What is the vapor pressure, in torr, of the solution formed bydissolving 50.0 g of glycerin in 500.0 g of water at 25 °C? The vapor pressure of pure water at this temperature is23.8 torr.
The Henry's Law constant of methyl bromide, CH3Br, is k = 0.159 mol/(L atm) at 25°C. What is the solubility of this compound in water at 25°C and at a partial pressure of 406 mmHg?
159
Substance A (P° = 145 torr) and B (P° = 212 torr) form a real solution. When you make a solutionthat has a 4:1 mole ratio of A:B, the resulting vapor pressure of the solution is 173 torr. Doesthe solution display a negative or positive deviation from Raoult’s Law? What does this tellyou about the intermolecular interactions between A and B vs pure A and pure B?
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