Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
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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
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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,...
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Similar questions
Sulfur, in its cyclic molecular form having the formula S8, is an unusual element in that the solid form has two easily accessible solid phases. The rhombic crystal solid is stable at temperatures lower than 95.5C, and has a density of 2.07g/cm3. The monoclinic phase, stable at temperatures higher than 95.5C and less than the melting point of sulfur, has a density of 1.96g/cm3. Use equation 6.10 to estimate the pressure necessary to make rhombic sulfur the stable phase at 100C if the entropy of transition is 1.00J/molK. Assume that transS does not change with changing conditions.
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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 )?
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5.35. The densities of graphite and diamond are and , respectively. Using the expression
and equation 5.14, estimate the pressure necessary for to equal zero. What is the stable high-pressure solid phase of carbon?
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Consider the phase diagram of sulfur in the previous exercise. If one starts at 25C and 1atm pressure which is equal to 1bar and increases the temperature, comment on the entropy change as the sulfur goes from rhombic to monoclinic solid phases. Is it positive or negative? On the basis of the second law of thermodynamics, is the phase transition expected to be spontaneous?
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The 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.
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Identify the phase transitions that occur for this system as the temperature varies at constant pressure. Determine the coexistence temperatures and the temperature range over which each phase is stable.
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6.31. If it takes mega bars of pressure to change the melting point of a substance from to for a change in molar volume of , what is the heat of fusion of the substance?
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At 20.0C, the vapor pressure of ethanol is 43.7mmHg. If its enthalpy of vaporization is 38.6kJ/mol, at what temperature would the vapor pressure equal 250.0mmHg?
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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?
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Use equations 4.21 and 4.25 to explain why H and G vary much more with pressure for a gas than they do for a solid and a liquid.
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At the triple point of a substance, the vapor pressures of the solid and the liquid phase are the same. Using the Clausius-Clapeyron equation for each combination of phases, one can show that the temperature of the triple point, Ttp, is Ttp=fusHRlnpliqpsol+vapHTliqsubHTsol where the data points pliq, Tliq and psol, Tsol are the vapor pressure and temperature data for the liquid and solid phases, respectively. a Given these data, calculate Ttp for iodine, I2. fusH15.52kJ/molsubH57.09kJ/molvapH41.57kJ/mol psolat364K10.00torrpliqat410K200.0torr b Calculate the vapor pressure of I2 at the triple point using the Clausius-Clapeyron equation and the fact that the normal boiling point of I2 is 457.4K.
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