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 6.24E
Interpretation Introduction
Interpretation: The applicability of
Concept introduction: Entropy is a
The randomness of the molecules increases when solid is melted and liquid is converted into vapor state. As in vapor state particles move freely because they are at larger distances from each other.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Would more or less heat be evolved by burning gaseous nitro methane versus liquid nitro methane? And why?
A certain liquid has a vapor pressure of 92.0 Torr92.0 Torr at 23.0 ∘C23.0 ∘C and 335.0 Torr335.0 Torr at 45.0 ∘C.45.0 ∘C.
Calculate the value of Δ?∘vapΔHvap∘ for this liquid.
In 1870 Ludwig Boltzmann gave us this equation:
What is the meaning of these terms?
Select all that are true.
W = work
S = k In (W)
k is the Boltzmann constant. k = 1.38 x10-23J/K
k = R/NA, The gas constant divided by Avogadro's Number
OS Spontaneous energy
=
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
- For a liquid, which would you expect to be larger, Sfusion or Sevaporation? Why?arrow_forward9.23 Which system does not work: (a) E=436J , q=400J ; or E=317J , q=347J ?arrow_forwardPhosphorus exists in multiple solid phases, including two known as red phosphorus and white phosphorus. (a) Based on their respective heats of formation, which form of phosphorus is defined as the standard state? (b) Now consider the phase transition between white and red phosphorous: P4(s, white4 P(s, red). Use data from Appendix E to determine which form of phosphorous is actually more stable at 25C. (Your result should reveal that phosphorus is an exception to the usual convention for defining the standard state.) (c) Is the same form of the solid more stable at all temperatures? If not, what temperatures are needed to make the other form more stable?arrow_forward
- Four alcohols have the formula C4H9OH: 1-butanol, 2-butanol or sec-butanol, isobutanol or 2-methyl-2-propanol. They are examples of isomers, or compounds that have the same molecular formula but different molecular structures. The following table gives data on the isomers: Compound vapH(kJ/mol) Normal boiling point (C) 1-Butanol 45.90 117.2 2-Butanol 44.82 99.5 Isobutanol 45.76 108.1 tert-Butanol 43.57 82.3 Using the Clausius-Clapeyron equation, rank the isomers of butanol in order of decreasing vapor pressure at 25C. Does the ranking agree with any conventional wisdom based on the vapH or the normal boiling points?arrow_forwardWould the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.arrow_forwardSuppose you have a system made up of water only, with the container andeverything beyond being the surroundings. Consider a process in which the water is first evaporated and then condensed back into its original container. Is this two-step process necessarily reversible?arrow_forward
- 6 .If 2.1g of 100.0C steam begins to condense on a container of liquid water at 25.0C and they eventually reach the same temperature of 46.7C what was the mass of liquid water in the container? *Assume all heat from the steam cooling goes into the liquid water.*arrow_forwardA 0.305 mol0.305 mol sample of N2(g),N2(g), initially at 298 K298 K and 1.00 atm,1.00 atm, is held at constant pressure while enough heat is applied to raise the temperature of the gas by 11.1 K.11.1 K. Calculate the amount of heat ?q required to bring about this temperature change, and find the corresponding total change in the internal energy Δ?ΔU of the gas. Assume that the constant‑pressure molar specific heat for N2(g),N2(g), which consists of linear molecules, is equal to 7?/2,7R/2, where ?=8.3145 J/(mol·K)R=8.3145 J/(mol·K) is the ideal gas constant. ?=? Δ?= ?arrow_forward9. The amount of energy in form of heat needed to raise its temperature by 1 degree celcius of 1g of a sustance is also known as heat capacity A.True B. Falsearrow_forward
- 2.00-mol of a monatomic ideal gas goes from State A to State D via the path A→B→C→D: State A PA=13.0atm, VA=11.50L State B PB=13.0atm, VB=6.00L State C PC=21.5atm, VC=6.00L State D PD=21.5atm, VD=21.50L Assume that the external pressure is constant during each step and equals the final pressure of the gas for that step. Calculate q for this process. Calculate w for this process. Calculate ΔE for this process Calculate ΔH for this process.arrow_forwardA certain liquid has a vapor pressure of 92.0 Torr92.0 Torr at 23.0 ∘C23.0 ∘C and 370.0 Torr370.0 Torr at 45.0 ∘C.45.0 ∘C. Calculate the value of Δ?∘vapΔHvap∘ for this liquid. Answer at kj/mol. Calculate the normal boiling point of this liquid.arrow_forward2) Given the following data for graphite and diamond at 298K. S°(diamond) = 0.58 cal/mole deg S°(graphite) = 1.37 cal/mole deg DHf° CO2(from graphite) = -94.48 kilocalories/mole DHf° CO2(from diamond) = -94.03 kilocalories/mole R in calories = 1.986 calories mol -1 K-1 Consider the change: C(graphite) → C(diamond) at 298K and 1 atmosphere. (a) What are the values of DS° and DH° for the conversion of graphite to diamond? (b) Perform a calculation to show whether it is thermodynamically feasible to produce diamond from graphite at 298K and 1 atmosphere. (c) For the reaction, calculate the equilibrium constant Keq at 298K Please answer A, B, and C. Thank youarrow_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,
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Chemistry for Engineering StudentsChemistryISBN:9781285199023Author: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
Physical Chemistry
Chemistry
ISBN:9781133958437
Author:Ball, David W. (david Warren), BAER, Tomas
Publisher:Wadsworth Cengage Learning,
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781285199023
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