Chemistry & Chemical Reactivity
10th Edition
ISBN: 9781337399074
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 11, Problem 13PS
Answer the following questions using Figure 11.12:
- (a) What is the approximate equilibrium vapor pressure of water at 60 °C? Compare your answer with the data in Appendix G.
- (b) At what temperature does water have an equilibrium vapor pressure of 600 mm Hg?
- (c) Compare the equilibrium vapor pressures of water and ethanol at 70 °C. Which is higher?
Figure 11.12 Vapor pressure curves for diethyl ether [(C2H3)2O], ethanol (C2H5OH), and water. Each curve represents conditions of T and P of which the two phases, liquid and vapor, are in equilibrium. These compounds exist as liquids for temperatures and pressures to the left of the curve and as gases under conditions to the right of the curve. (See Appendix G for vapor pressures for water of various temperatures.)
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
Select the compound that will have the lower equilibrium vapor pressure based on
predicted intermolecular forces.
pentane (C5H12)
phosphorus tribromide
For a compound the ΔHofus is 11.7 kJ/mol and the ΔSofus is 38.9 J/mol∙K. What is the melting point (in oC)?
3. (a) The Lattice enthalpy for the solid ionic compound AgBr is +900. kJ/mole.
Write the chemical equation that corresponds to the Lattice Enthalpy for AgBr(s) in the space above.
Then explain in your own words why this is a large positive number.
(b) The hydration enthalpy for AgBr is -821 kJ/mole.
Write the chemical equation that corresponds to the Hydration Enthalpy for AgBr(s) in the space above.
Then explain in your own words why this is a large negative number.…
Chapter 11 Solutions
Chemistry & Chemical Reactivity
Ch. 11.2 - Which should have the more negative hydration...Ch. 11.3 - Using structural formulas, describe the hydrogen...Ch. 11.4 - Prob. 11.3CYUCh. 11.5 - Prob. 11.4CYUCh. 11.6 - The molar enthalpy of vaporization of methanol,...Ch. 11.6 - Prob. 11.6CYUCh. 11.6 - Prob. 1.1ACPCh. 11.6 - Prob. 1.2ACPCh. 11.6 - Prob. 2.1ACPCh. 11.6 - Prob. 2.2ACP
Ch. 11 - Prob. 1PSCh. 11 - Intermolecular forces: What type of forces must be...Ch. 11 - Prob. 3PSCh. 11 - Prob. 4PSCh. 11 - Considering intermolecular forces in the pure...Ch. 11 - Considering intermolecular forces in the pure...Ch. 11 - Prob. 7PSCh. 11 - Which of the following compounds would be expected...Ch. 11 - Prob. 9PSCh. 11 - When salts of Mg2+, Na+, and Cs+ are placed in...Ch. 11 - Prob. 11PSCh. 11 - The enthalpy of vaporization of liquid mercury is...Ch. 11 - Answer the following questions using Figure 11.12:...Ch. 11 - Answer the following questions using Figure 11.12:...Ch. 11 - Prob. 15PSCh. 11 - Refer to Figure 11.12 to answer these questions:...Ch. 11 - Which member of each of the following pairs of...Ch. 11 - Place the following four compounds in order of...Ch. 11 - Prob. 19PSCh. 11 - You are comparing three different substances, A,...Ch. 11 - Equilibrium vapor pressures of benzene, C6H6, at...Ch. 11 - Prob. 22PSCh. 11 - Can carbon monoxide (Tc = 132.9 K; Pc = 34.5 atm...Ch. 11 - Methane (CH4) cannot be liquefied at room...Ch. 11 - What is surface tension? Give an example...Ch. 11 - What factors affect the viscosity of a substance?...Ch. 11 - If a piece of filter paper (an absorbent paper...Ch. 11 - When water is placed in a buret it forms a concave...Ch. 11 - Prob. 29GQCh. 11 - What types of intermolecular forces are important...Ch. 11 - Which of the following salts, Li2SO4 or Cs2SO4, is...Ch. 11 - Prob. 32GQCh. 11 - Prob. 33GQCh. 11 - Prob. 34GQCh. 11 - Rank the following compounds in order of...Ch. 11 - Prob. 36GQCh. 11 - Prob. 37GQCh. 11 - The following data are the equilibrium vapor...Ch. 11 - Prob. 39ILCh. 11 - A hand boiler can be purchased in toy stores or at...Ch. 11 - Prob. 41ILCh. 11 - Prob. 42ILCh. 11 - Acetone, CH3COCH3, is a common laboratory solvent....Ch. 11 - Cooking oil floats on top of water. From this...Ch. 11 - Liquid ethylene glycol, HOCH2CH2OH, is one of the...Ch. 11 - Liquid methanol, CH3OH, is placed in a glass tube....Ch. 11 - Account for these facts: (a) Although ethanol...Ch. 11 - Prob. 48SCQCh. 11 - Prob. 49SCQCh. 11 - Prob. 50SCQCh. 11 - Prob. 51SCQCh. 11 - Prob. 52SCQCh. 11 - A fluorocarbon, CF4, has a critical temperature of...Ch. 11 - Prob. 55SCQCh. 11 - List four properties of liquids that are directly...Ch. 11 - List the following ions in order of hydration...Ch. 11 - Prob. 59SCQCh. 11 - An 8.82-g sample of Br2 is placed in an evacuated...Ch. 11 - Polarizability is defined as the extent to which...Ch. 11 - Prob. 62SCQCh. 11 - A pressure cooker (a kitchen appliance) is a pot...Ch. 11 - Vapor pressures of NH3() at several temperatures...Ch. 11 - Prob. 65SCQCh. 11 - Prob. 66SCQCh. 11 - Prob. 67SCQ
Additional Science Textbook Solutions
Find more solutions based on key concepts
45. Calculate the mass of nitrogen dissolved at room temperature in an 80.0-L home aquarium. Assume a total pre...
Chemistry: Structure and Properties (2nd Edition)
Single penny tossed 20 times and counting heads and tails: Probability (prediction): _______/20 heads ________/...
Laboratory Manual For Human Anatomy & Physiology
2. Which of the following is the best example of the use of a referent? _
a. A red bicycle
b. Big as a dump tru...
Physical Science
The validity of a scientific law.
Physical Universe
56. Global Positioning System. Learn more about the global positioning system and its uses. Write a short repo...
The Cosmic Perspective (8th Edition)
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Are changes in state physical or chemical changes? Explain. What type of forces must be overcome to melt or vaporize a substance (are these forces intramolecular or intermolecular)? Define the molar heat of fusion and molar heat of vaporization. Why is the molar heat of vaporization of water so much larger than its molar heat of fusion? Why does the boiling point of a liquid vary with altitude?arrow_forwardMaple syrup sap is 3% sugar (sucrose) and 97% water bymass. Maple syrup is produced by heating the sap toevaporate a certain amount of the water. (a) Describe what happens to the composition and boilingpoint of the solution as evaporation takes place. (b) A rule of thumb among maple syrup producers is thatthe finished syrup should boil about 4 C higher than theoriginal sap being boiled. Explain the chemistry behindthis guideline. (c) If the finished product boils 4 C higher than the originalsap, calculate the concentration of sugar in the finalproduct. Assume that sugar is the only solute and theoperation is done at 1 atm pressure.arrow_forward3. (a) The Lattice enthalpy for the solid ionic compound AgBr is +900. kJ/mole. Write the chemical equation that corresponds to the Lattice Enthalpy for AgBr(s) in the space above. Then explain in your own words why this is a large positive number. (b) The hydration enthalpy for AgBris -821 kJ/mole. Write the chemical equation that corresponds to the Hydration Enthalpy for AgBr(s) in the space above. Then explain in your own words why this is a large negative number. (c) Would you expect this compound to be soluble in water? Why/Why not? Calculate anything you need in order to figure this out, and explain your answer.arrow_forward
- 8. (a) Use the Clausius-Clapeyron equation and calculate the vapor pressure (mm Hg) of fluoroethane at -80 °C, given that the vapor pressure is 400. mm Hg at a temperature of -46 °C. The enthalpy of vaporization of fluoroethane is 23.0 kJ/mol. (b) Calculate the enthalpy of vaporization for a compound if its vapor pressure is 70 mm Hg at -50 °C and 323 mm Hg at -28 °C.arrow_forwardSelect the compound that will have the higher equilibrium vapor pressure based on predicted intermolecular forces. pentane (C5H12) iodine pentafluoridearrow_forwardDiethyl ether has a ΔH(vap)° of 29.1 kJ/mol and a vapor pres-sure of 0.703 atm at 25.0° C. What is its vapor pressure at 95.0° C?arrow_forward
- Calculate the vapor pressure (in atm) of pure water at 80.0°C. For water, ΔHvap = 40.7 kJ/mol, R = 8.314 J/K-molarrow_forwardAnswer the following question about an aqueous solution of tetrahydrofuran (C4H8O)with a concentration of 4.20 molal. The enthalpy of vaporization of tetrahydrofuran is 445.9 J/g. How much energy is required to convert the amount of tetrahydrofuran in the solution to vapor?arrow_forwardDiethyl ether has a ΔHvap of 29.1 kJ/mol and a vapor pressure of 0.703 atm at 25.0°C. What is its vapor pressure at 83.0°C?arrow_forward
- 60. Complete the following partial ICE tables. (b) 4NH3 (?) + 3O2(?)+⇌ 2N2 (?)+ 6H2O (?) Change ----------- +x ---------- -----------arrow_forward2. Density of AgBr is 6.47 x 10 kg/m. AgBr has fcc lattice and molecular weight of AgCl is 187.77 g/mol. Calculate lattice constant (a) for AgBr.arrow_forward2. The boiling point of methanol is 338 K. What is the vapor pressure of methanol at 250 K, given that AHwap = 35 kJ/mol?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Chemical Equilibria and Reaction Quotients; Author: Professor Dave Explains;https://www.youtube.com/watch?v=1GiZzCzmO5Q;License: Standard YouTube License, CC-BY