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 6.24E
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.
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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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- Phosphorus 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_forwardWhat is the boiling point for HCN (in kelvin) from the data provided?_________Karrow_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
- Is entropy increased or decreased in boiling water?arrow_forwardCalculate the molar enthalpy of vaporization and normal boiling point of a liquid that follows Trouton's rule, which states that the vapor pressure of a liquid near its normal boiling point increases by about 15 mmHg for every 1°C increase in temperature.arrow_forward) What is ΔH° for the following phase change?NaCl(s) → NaCl(l)Substance ΔH°f (kJ/mol)NaCl(s) –411.12NaCl(l) –385.92a. 797.04 kJb. 25.20 kJc. –797.04 kJd. –25.20 kJe. 0 kJarrow_forward
- Arguably one of the most fundamental concepts in physical science is that of the second law of thermodynamics. Summarize the second law and make sure to include the two key aspects of the second law.arrow_forwardHow much energy is required to heat 100.0 g H2O from a liquid at 20.0°C to a complete gas at 100 °C? The following physical data may be useful. ΔH vap = 40.7 kJ/mol; Cs,H2O = 4.18 J/g. °C 139 kJ 33.7 kJ 259 kJ 151 kJ 225 kJarrow_forwardThe normal boiling point of Br2(l)Br2(l) is 58.8 ∘C∘C, and its molar enthalpy of vaporization is ΔHvapΔHvap = 29.6 kJ/molkJ/mol. Calculate the value of ΔSΔS when 2.00 molmol of Br2(l)Br2(l) is vaporized at 58.8 ∘C∘C.arrow_forward
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