References Use the References to access important values if needed for this question. Consider the reaction: 3Fe2O3 (s) + H2(g) →2Fe3O4 (s) + H2O(9) Using standard thermodynamic data at 298 K, calculate the entropy change for the surroundings when 1.62 moles of Fe2O3 (s) react at standard conditions. Substance AH (kJ/mol) AS Fe2O3(s) -824.2 H₂ (9) 0.0 Fe3O4(s) -1118.4 H₂O(g) 241.8 J/K surroundings Submit Answer

References Use the References to access important values if needed for this question. Consider the reaction: 3Fe2O3 (s) + H2(g) →2Fe3O4 (s) + H2O(9) Using standard thermodynamic data at 298 K, calculate the entropy change for the surroundings when 1.62 moles of Fe2O3 (s) react at standard conditions. Substance AH (kJ/mol) AS Fe2O3(s) -824.2 H₂ (9) 0.0 Fe3O4(s) -1118.4 H₂O(g) 241.8 J/K surroundings Submit Answer

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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Explain why the statement No process is 100 efficient is not the best statement of the second law of thermodynamics.
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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)
Define the following: a. spontaneous process b. entropy c. positional probability d. system e. surroundings f. universe
10.69 If a sample of air were separated into nitrogen and oxygen molecules (ignoring other gases present), what would be the sign of for this process? Explain your answer. The next four questions relate to the following paragraph [Frank L. Lambert, Journal of Chemical Education, 76(10), 1999, 1385]. "The movement of macro objects from one location to another by an external agent involves no change in the objects' physical (thermodynamic) entropy. The agent of movement undergoes a thermodynamic entropy increase in the process."
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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.
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).
For the reaction NO(g)+NO2(g)N2O3(g) , use tabulated thermodynamic data to calculate H and S. Then use those values to answer the following questions. (a) Is this reaction spontaneous at 25°C? Explain your answer. (b) If the reaction is not spontaneous at 25°C, will it become spontaneous at higher temperatures or lower temperatures? (c) To show that your prediction is accurate, choose a temperature that corresponds to your prediction in part (b) and calculate G . (Assume that both enthalpy and entropy are independent of temperature.)
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)
Calculate the entropy change for each of these processes. thereby verifying the predictions made in Conceptual Exercise 16.4. (a) 2 CO2(g) 2 CO(g) + O2(g) (b) NaCl(s) NaCl(aq) (c) MgCO3(s) MgO(s) + CO2(g)
Consider the reaction of 2 mol H2(g) at 25C and 1 atm with 1 mol O2(g) at the same temperature and pressure to produce liquid water at these conditions. If this reaction is run in a controlled way to generate work, what is the maximum useful work that can be obtained? How much entropy is produced in this case?

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