Item 1I Review Constants | Periodic TableElemental carbon usually exists in one of two forms: graphite or diamond. It is generally believed that diamonds last forever. The tableshows the standard enthalpy of formation (AH:) and the standard molar entropy (S°) values for diamond and graphite.SubstanceΔΗΡ (kJ/mol)S° (J/mol - K)Cgraphite5.740Cdiamond1.8972.38Part AWhat is the standard Gibbs free energy for the transformation of diamond to graphite at 298 K?CdiamondCgraphiteExpress your answer to three significant figures and include the appropriate units.> View Available Hint(s)ValueUnitsAGn

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Item 1 I Review | Constants | Periodic Table Elemental carbon usually exists in one of two forms: graphite or diamond. It is generally believed that diamonds last forever. The table shows the standard enthalpy of formation (AH:) and the standard molar entropy (S°) values for diamond and graphite. Substance AH: (kJ/mol) S° (J/mol K) Cgraphite 5.740 Caiamond 1.897 2.38 Part A What is the standard Gibbs free energy for the transformation of diamond to graphite at 298 K? Cdiamond→Cgraphite Express your answer to three significant figures and include the appropriate units. > View Available Hint(s) ? AGm = Value Units

Item 1 I Review | Constants | Periodic Table Elemental carbon usually exists in one of two forms: graphite or diamond. It is generally believed that diamonds last forever. The table shows the standard enthalpy of formation (AH:) and the standard molar entropy (S°) values for diamond and graphite. Substance AH: (kJ/mol) S° (J/mol K) Cgraphite 5.740 Caiamond 1.897 2.38 Part A What is the standard Gibbs free energy for the transformation of diamond to graphite at 298 K? Cdiamond→Cgraphite Express your answer to three significant figures and include the appropriate units. > View Available Hint(s) ? AGm = Value Units

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 93QRT: The standard molar entropy of iodine vapor, I2(g), is 260.7 J Kl mol-1 and the standard molar...

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The 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.
What is the second law of thermodynamics? For any process, there are four possible sign combinations for Ssys and Ssurr. Which sign combination(s) always give a spontaneous process? Which sign combination(s) always give a non-spontaneous process? Which sign combination(s) may or may not give a spontaneous process?
Consider two processes: sublimation of I2(s) and melting of I2(s) (Note: the latter process can occur at the same temperature but somewhat higher pressure). I2(s)I2(g)I2(s)I2(l) Is S positive or negative in these processes? In which of the processes will the magnitude of the entropy change be greater?
The free energy change, G, for a process at constant temperature and pressure is related to Suniv and reflects the spontaneity of the process. How is G related to Suniv? When is a process spontaneous? Nonspontaneous? At equilibrium? G is a composite term composed of H, T, and S. What is the G equation? Give the four possible sign combinations for H and S. What temperatures are required for each sign combination to yield a spontaneous process? If G is positive, what does it say about the reverse process? How does the G = H TS equation reduce when at the melting-point temperature of a solid-to-liquid phase change or at the boiling-point temperature of a liquid-to-gas phase change? What is the sign of G for the solid-to-liquid phase change at temperatures above the freezing point? What is the sign of G for the liquid-to-gas phase change at temperatures below the boiling point?
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)
The standard molar entropy of iodine vapor, I2(g), is 260.7 J Kl mol-1 and the standard molar enthalpy of formation is 62.4 kJ/mol. a) Calculate the entropy change for vaporization of 1 mol of solid iodine (use data from Table 16.1 or Appendix J). b) Calculate the enthalpy change for sublimation of iodine. c) Assuming that rSdoes not change with temperature, estimate the temperature at which iodine would sublime (change directly from solid to gas).
Many plastic materials are organic polymers that contain carbon and hydrogen. The oxidation of these plastics in air to farm carbon dioxide and water is a spontaneous process; however, plastic materials tend to persist in the environment. Explain.
What is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the formation of hydrogen sulfide from the elements? H2(g)+18S8(s)H2S(g)
Explain why absolute entropies can be measured.
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 kJ
10.104 (a) When a chemical bond forms, what happens to the entropy of the system? (b) Thermodynamically, what allows any bond formation to occur? (c) What do your answers to parts (a) and (b) suggest must be true about the formation of chemical bonds for the octet rule to hold?
In a spontaneous process, S(universe) is (a) 0 (b) = 0 (c) 0