Consider the reaction: 2SO2(g) + O2(g) → 2SO3 (9) Using standard absolute entropies at 298 K, calculate the entropy change for the system when 1.63 moles of SO2 (g) react at standard conditions. J Substance So K mol SO3 (9) 256.8 SO2(g) 248.2 02 (9) 205.1 J/K ASO system Submit Answer Retry Entire Group 9 more group attempts remaining

Consider the reaction: 2SO2(g) + O2(g) → 2SO3 (9) Using standard absolute entropies at 298 K, calculate the entropy change for the system when 1.63 moles of SO2 (g) react at standard conditions. J Substance So K mol SO3 (9) 256.8 SO2(g) 248.2 02 (9) 205.1 J/K ASO system Submit Answer Retry Entire Group 9 more group attempts remaining

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter10: Entropy And The Second Law Of Thermodynamics

Section: Chapter Questions

Problem 10.8PAE: In the thermodynamic definition of a spontaneous process, why is it important that the phrase...

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The synthesis of glucose directly from CO2 and H2O and the synthesis of proteins directly from amino acids are both non-spontaneous processes under standard conditions. Yet it is necessary for these to occur for life to exist. In light of the second law of thermodynamics, how can life exist?
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Explain why absolute entropies can be measured.
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It has been demonstrated that buckminsterfullerene (C60), another allotrope of carbon (Section 2.3), may be converted into diamond at room temperature and 20,000 atmospheres pressure (about 2 GPa). The standard enthalpy of formation, fH, for buckminsterfullerene is 2320 kJ/mol at 298.2 K. a. Calculate rH for the conversion of C60 to diamond at standard state conditions and 2982 K. b. Assuming that the standard entropy per mole of carbon in both C60 and diamond is comparable (both about 23 J/K mol), is the conversion of C60 to diamond product-favoredat room temperature?
According to Lambert, leaves lying in the yard and playing cards that are in disarray on a table have not undergone an increase in their thermodynamic entropy. Suggest another reason why leaves and playing cards may not be a good analogy for the entropy of a system containing, for example, only H2O molecules or only O2 molecules.
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What 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)
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