Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
expand_more
expand_more
format_list_bulleted
Question
Chapter 6, Problem 6.41E
Interpretation Introduction
Interpretation:
The relationship to the change in the pressure of the vaporized compound if the temperature is increased linearly is to be predicted. Also, the reason as to why it is important to be careful when vaporizing materials at high temperatures is to be explained.
Concept introduction:
Vapor pressure is defined as the pressure exerted by a vapor in
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
19) Clausius-Clapeyron
equation
a) Consider the Clapeyron equation for a vaporization process. Since the molar
volume of a gas is much larger than the molar volume of a liquid, the change in
volume can be simplified by the gas volume. Using this information, derive the
Clausius-Clapeyron equation from the Clapeyron equation under the assumption
that the vapor behaves like an ideal gas and that Hap is constant over a small
range.
Hint: Use n = 1 mol and therefore the molar enthalpy of vaporization 4Hvap,molar
b) Use the Clausius-Clapeyron equation to determine the molar enthalpy of
vaporization 4Hvap,molar of ethanol, given the following values for the vapor
pressure: p₁ (349.05 K) = 0.93846 bar and p₂(350.75 K) = 0.99698 bar.
The relative humidity of air equals the ratio of the partial pressure of water in the air to the equilibrium vapor pressure of
water at the same temperature times 100%. If the relative humidity of the air is 58% and its temperature is 68 of, how
many moles of water are present in a room measuring 12 ft x 10 ft x 8 ft? The vapor pressure of water at 68 oF is 17.54 torr.
The answer is 20, but for some reason I keep getting 15.127moles
Chapter 6 Solutions
Physical Chemistry
Ch. 6 - Prob. 6.1ECh. 6 - Prob. 6.2ECh. 6 - Prob. 6.3ECh. 6 - Prob. 6.4ECh. 6 - Prob. 6.5ECh. 6 - Prob. 6.6ECh. 6 - Prob. 6.7ECh. 6 - Prob. 6.8ECh. 6 - 6.9. Identify and explain the sign on in equation...Ch. 6 - 6.10. Use Hess’s law to prove that .
Ch. 6 - 6.11. Calculate the amount of heat necessary to...Ch. 6 - Prob. 6.12ECh. 6 - Assume that the vapH of an evaporating liquid...Ch. 6 - 6.14. As a follow-up to the previous exercise,...Ch. 6 - Prob. 6.15ECh. 6 - 6.16. What is for isothermal conversion of liquid...Ch. 6 -
6.17. Estimate the melting point of nickel, Ni,...Ch. 6 -
6.18. Estimate the boiling point of platinum, Pt,...Ch. 6 - Prob. 6.19ECh. 6 - Prob. 6.20ECh. 6 - 6.21. What assumption is used in the integration...Ch. 6 - Prob. 6.22ECh. 6 - Sulfur, in its cyclic molecular form having the...Ch. 6 - Prob. 6.24ECh. 6 - 6.25. Phosphorus exists as several allotropes that...Ch. 6 - Prob. 6.26ECh. 6 - 6.27. What is higher for a substance: its normal...Ch. 6 - 6.28. Elemental gallium is another substance whose...Ch. 6 - Prob. 6.29ECh. 6 - Consider the sulfur solid-state phase transition...Ch. 6 - 6.31. If it takes mega bars of pressure to change...Ch. 6 - Prob. 6.32ECh. 6 - Four alcohols have the formula C4H9OH: 1-butanol,...Ch. 6 - Prob. 6.34ECh. 6 - At 20.0C, the vapor pressure of ethanol is...Ch. 6 - Prob. 6.36ECh. 6 - Prob. 6.37ECh. 6 - Ethanol has a density of 0.789g/cm3 and a vapor...Ch. 6 - Prob. 6.39ECh. 6 - Prob. 6.40ECh. 6 - Prob. 6.41ECh. 6 - 6.42. At what pressure does the boiling point of...Ch. 6 - Prob. 6.43ECh. 6 - Prob. 6.44ECh. 6 - Prob. 6.45ECh. 6 - Prob. 6.46ECh. 6 - Prob. 6.47ECh. 6 - 6.48. Explain how glaciers, huge masses of solid...Ch. 6 - Prob. 6.49ECh. 6 - Prob. 6.50ECh. 6 - Prob. 6.51ECh. 6 - Prob. 6.52ECh. 6 - Prob. 6.53ECh. 6 - Prob. 6.54ECh. 6 - Prob. 6.55ECh. 6 - Prob. 6.56ECh. 6 - Prob. 6.57ECh. 6 - Use the phase diagram of water in Figure 6.6 and...Ch. 6 - Prob. 6.59ECh. 6 - Prob. 6.60ECh. 6 - At the triple point of a substance, the vapor...Ch. 6 - Prob. 6.62ECh. 6 - Prob. 6.63ECh. 6 - Prob. 6.64ECh. 6 - Prob. 6.65ECh. 6 - Prob. 6.66ECh. 6 - The phase diagram for elemental sulfur is shown in...Ch. 6 - Consider the phase diagram of sulfur in the...Ch. 6 - Prob. 6.69ECh. 6 - Rearrange the Clausius-Clapeyron equation,...
Knowledge Booster
Similar questions
- 6.27. What is higher for a substance: its normal boiling point (where the surrounding pressure is ) or the standard boiling point (where the surrounding pressure is )?arrow_forwardThe vapor pressures of benzene and and 1,1 dichloroethane at 25.0C are 94.0 and 224.9mmHg, respectively. What does a plot of total pressure versus the mole fraction of benzene in the vapor look like? What does a plot of total pressure versus the mole fraction of 1,1 chloroethane look like? Compare these plots with your plots from exercise 7.87.arrow_forwardConsider the following data for the vapor pressure of diethyl ether, a widely used anesthetic in the early days of surgery. Follow the instructions in Question 13 to estimate the heat of vaporization of diethyl ether.arrow_forward
- Given the following data about xenon, normalboilingpoint=108Cnormalmeltingpoint=112Ctriplepoint=121Cat281mmHgcriticalpoint=16.6Cat58atm (a) Construct an approximate phase diagram for xenon. (b) Estimate the vapor pressure of xenon at -115C. (c) Is the density of solid Xe larger than that for liquid Xe?arrow_forwardDescribe the behavior of a liquid and its vapor in a closed vessel as the temperature increases.arrow_forwardIf you've ever opened a bottle of rubbing alcohol or other solvent on a warm day, you may have heard a little “whoosh” as the vapor that had built up above the liquid escapes. Describe on a microscopic basis how a vapor pressure builds up in a closed container above a liquid. What processes in the container give rise to this phenomenon?arrow_forward
- Use the phase diagram of water in Figure 6.6 and count the total number of phase transitions that are represented.arrow_forwardThe graph below is obtained when a liquid metal is cooled at a constant rate to the temperature at which it solidifies and the solid is cooled further. Account for the shape of this graph. Would all substances exhibit similar graphs?arrow_forwardSatellites in space often suffer from vacuum welding, in which two metal parts in contact tend to stick together more than expected over a period of time. Why does this phenomenon occur in space and not on Earth?arrow_forward
- 6.25. Phosphorus exists as several allotropes that have varying properties. The enthalpy of transition from white P to red P, , is . The densities of white and red phosphorus are and , respectively. At what temperature does white phosphorus become the stable phase at of pressure? Assume the formula for phosphorus is .arrow_forwardIt is a hot summer day, and Chris wants a glass of lemonade. There is none in the refrigerator, so a new batch is prepared from freshly squeezed lemons. When finished, there are 175g of lemonade at 23C. That is not a very refreshing temperature, so it must be cooled with ice. But Chris doesnt like ice in lemonade Therefore, just enough ice is used to cool the lemonade to 5C. Of course, the ice will melt and reach the same temperature. If the ice starts melting at 8C, and if the specific heat of lemonade is the same as that of water, how many grams of ice does Chris use? Assume there is no heat transfer to or from the surroundings. Answer in two significant figures.arrow_forwardWhat are the two ways in which the escape of high-energy molecules from the surface of a liquid during the process of evaporation affects the liquid?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Physical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,
Introductory Chemistry: An Active Learning Approa...ChemistryISBN:9781305079250Author:Mark S. Cracolice, Ed PetersPublisher:Cengage Learning
Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
World of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage Learning
Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Physical Chemistry
Chemistry
ISBN:9781133958437
Author:Ball, David W. (david Warren), BAER, Tomas
Publisher:Wadsworth Cengage Learning,
Introductory Chemistry: An Active Learning Approa...
Chemistry
ISBN:9781305079250
Author:Mark S. Cracolice, Ed Peters
Publisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
World of Chemistry, 3rd edition
Chemistry
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Brooks / Cole / Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning