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A bottle at 325 K contains an ideal gas at a pressure of
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Chapter 2 Solutions
Thermodynamics, Statistical Thermodynamics, & Kinetics
- Which of the following quantities can be taken to be independent of temperature? independent of pressure? (a) H for a reaction (b) S for a reaction (c) G for a reaction (d) S for a substancearrow_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_forwardUse the two appropriate values of R to determine a conversion between L. atm and J.arrow_forward
- What are the two ways that a final chemical state of a system can be more probable than its initial state?arrow_forwardBenzoic acid, C6H5COOH, is a common standard used in bomb calorimeters, which maintain a constant volume. If 1.20 g of benzoic acid gives off 31, 723 J of energy when burned in the presence of excess oxygen and in a water bath having a temperature of 24.6 C, calculate q, w, H, and U for the reaction.arrow_forwardUse the data in Table 2.2 to determine Hp T for Ar at 0C and 1atm. Make any reasonable assumptions necessary.arrow_forward
- Consider 2.00 moles of an ideal gas that are taken from state A (PA = 2.00 atm, vA = 10.0 L) to state B (PB = 1.00 attn, VB = 30.0 L) by two different pathways: These pathways are summarized on the following graph of P versus V: Calculate the work (in units of J) associated with the two pathways. Is work a state function? Explain.arrow_forwardCalculate the work for the isothermal, reversible compressionof 0.245 moleof an idealgas going from 1.000L to 1.00 mL if the temperature were 95.0C.arrow_forwardWhy is equation2.37 written interms of CV and Cp and not c-v and c-p ?arrow_forward
- 6E. A 2.25 mole sample of CO,(g), for which C,.m=37.1 J/K at 298 K, expands reversibly and adiabatically from a volume of 4.50 L and a temperature of 298 K to a final volume of 32.5 L. Calculate the final temperature, q, w, AH and AU for the process. Assume that the gas behaves ideally and that C. is p.m constant over this temperature interval.arrow_forward5. One mole of a monatomic ideal gas is compressed adiabatically in a single stage with a constant opposing pressure equal to 10 atm. Initially the gas is at 27 °C and 1 atm pressure, the final pressure is 10 atm. How would the various quantities be affected if n moles were used instead of one mole? For a monatomic ideal gas. C₂ = Cv R. 2arrow_forwardInitially at 300 K and 10 atm pressure, 1 mol of a gas is allowed to expand adiabatically against a constant pressure of 4 atm until equilibrium is achieved. Assume the gas to be ideal with Cp,m = 28.58 + 1.76 x 10^-2 T(The units of T are K and the units of Cp,m are J K-1 mol-1.) Compute DU, DH, q and w.arrow_forward
- Physical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
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