Thermodynamics, Statistical Thermodynamics, & Kinetics
3rd Edition
ISBN: 9780321766182
Author: Thomas Engel, Philip Reid
Publisher: Prentice Hall
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Chapter 5, Problem 5.2CP
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Chapter 5 Solutions
Thermodynamics, Statistical Thermodynamics, & Kinetics
Ch. 5 - Under what conditions is S0 for a spontaneous...Ch. 5 - Why are Sfustion and Svaporization always...Ch. 5 - An ideal gas in thermal contact with the...Ch. 5 - Prob. 5.4CPCh. 5 - Prob. 5.5CPCh. 5 - You are told that S=0 for a process in which the...Ch. 5 - Under what conditions does the equality S=H/T...Ch. 5 - Is the following statement true or false? If it is...Ch. 5 - Prob. 5.9CPCh. 5 - One Joule of work is done on a system, raising its...
Ch. 5 - Prob. 5.11CPCh. 5 - An ideal gas undergoes an adiabatic expansion into...Ch. 5 - When a saturated solution of a salt is cooled, a...Ch. 5 - Prob. 5.14CPCh. 5 - Prob. 5.15CPCh. 5 - Prob. 5.16CPCh. 5 - Why is the efficiency of a Carnot heat engine the...Ch. 5 - Two vessels of equal volume, pressure and...Ch. 5 - Solid methanol in thermal contact with the...Ch. 5 - Can incandescent lighting be regarded as an...Ch. 5 - The Chalk Point, Maryland, generating station...Ch. 5 - An electrical motor is used to operate a Carnot...Ch. 5 - An air conditioner is a refrigerator with the...Ch. 5 - Prob. 5.5NPCh. 5 - The average heat evolved by the oxidation of...Ch. 5 - Prob. 5.9NPCh. 5 - The maximum theoretical efficiency of an internal...Ch. 5 - Prob. 5.11NPCh. 5 - Prob. 5.12NPCh. 5 - Prob. 5.13NPCh. 5 - Prob. 5.14NPCh. 5 - Prob. 5.15NPCh. 5 - Prob. 5.16NPCh. 5 - Prob. 5.17NPCh. 5 - Prob. 5.18NPCh. 5 - Prob. 5.19NPCh. 5 - Prob. 5.20NPCh. 5 - Prob. 5.21NPCh. 5 - Prob. 5.22NPCh. 5 - Prob. 5.23NPCh. 5 - Prob. 5.24NPCh. 5 - Prob. 5.25NPCh. 5 - Prob. 5.26NPCh. 5 - Under anaerobic conditions, glucose is broken down...Ch. 5 - Prob. 5.28NPCh. 5 - Prob. 5.29NPCh. 5 - Prob. 5.30NPCh. 5 - Prob. 5.31NPCh. 5 - Calculate Ssurroundings and Stotal for the...Ch. 5 - A refrigerator is operated by a 0.25-hp...Ch. 5 - Prob. 5.34NPCh. 5 - Between C and 100C, the heat capacity of Hg(l) is...Ch. 5 - Prob. 5.36NPCh. 5 - Prob. 5.37NPCh. 5 - Prob. 5.38NPCh. 5 - Prob. 5.39NPCh. 5 - Prob. 5.40NPCh. 5 - Prob. 5.41NPCh. 5 - Prob. 5.42NPCh. 5 - An ideal gas sample containing 1.75 moles for...Ch. 5 - Prob. 5.44NPCh. 5 - Prob. 5.45NP
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- Given the following information at 25C, calculate G at 25C for the reaction 2A(g)+B(g)3C(g) Substance Hf(kJ/mol) S(J/molK) A(g) 191 244 B(g) 70.8 300 C(g) 197 164 a 956 kJ b 956 kJ c 346 kJ d 346 kJ e 1.03 103 kJarrow_forwardWithout looking up their standard entropies in reference tables, identify which of the following lists the materials in order of increasing entropy. (a) H2O() NaCl(s) NH3(g) (b) H2O() NH3(g) NaCl(s) (c) NaCl(s) H2O() NH3(g) (d) NH3(g) H2O() NaCl(s)arrow_forwardFor the reaction BaCO3(s) BaO(s) + CO2(g), rG = +219.7 kJ/mol-rxn. Using this value and other data available in Appendix L, calculate the value of fG for BaCO3(s).arrow_forward
- Calculate the standard Gibbs free-energy change when SO3 forms from SO2 and O2 at 298 K. Why is sulfur trioxide an important substance to study? (Hint: What happens when it combines with water?)arrow_forwardWhat is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the synthesis of ammonia? 3H2(g) + N2(g) 2NH3(g)arrow_forwardDefine the following: a. spontaneous process b. entropy c. positional probability d. system e. surroundings f. universearrow_forward
- Solid NH4NO3 is placed in a beaker containing water at 25 C. When the solid has completely dissolved, the temperature of the solution is 23.5 C. (a) Was the process exothermic or endothermic? (b) Was the process spontaneous? (c) Did the entropy of the system increase? (d) Did the entropy of the universe increase?arrow_forwardFor the reaction TiCl2(s) + Cl2(g) TiCl4(), rG = 272.8 kj/mol-txn. Using this value and other data available in Appendix L, calculate the value of fG for TiCl2(s).arrow_forwardWhen calculating rSfromSvalues, it is necessary to look up all substances, including elements in their standard state, such as O2(g), H2(g), and N2(g). When calculating rHfrom rHvalues, however, elements in theirstandard state can be ignored. Why is the situation different forSvalues?arrow_forward
- Use the data in Appendix G to calculate the standard entropy change for H2(g) + CuO(s) H2O() + Cu(s)arrow_forwardWhat is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the explosive decomposition of TNT? Use your knowledge of TNT and the chemical equation, particularly the phases, to answer this question. (Thermodynamic data for TNT are not in Appendix G.) 2C7H5N3O6(s) 3N2(g) + 5H2O() + 7C(s) + 7CO(g)arrow_forwardThe standard molar entropy of methanol vapor, CH3OH(g), is 239.8 J K1 mol-1. (a) Calculate the entropy change for the vaporization of 1 mol methanol (use data from Table 16.1 or Appendix J). (b) Calculate the enthalpy of vaporization of methanol, assuming that rS doesnt depend on temperature and taking the boiling point of methanol to be 64.6C.arrow_forward
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