For the isothermal expansion of a gas into a vacuum,ΔE = 0, q = 0, and w = 0. (a) Is this a spontaneous process?(b) Explain why no work is done by the system duringthis process. (c) What is the “driving force” for the expansionof the gas: enthalpy or entropy?

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Q: How Gibbs free energy is determined by the volume of the substance ?

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Q: At what temperatures will a reaction be spontaneous if ΔrH° = +62.4 kJ and ΔrS° = +301 J/K?

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Q: Given ΔHrxn∘= −135 kJ, ΔS∘rxn= −263 J/K, & T= 299 K, will the reaction be spontaneous?

A: Given: ΔHrxn∘= −135 kJ ΔS∘rxn= −263 J/K T= 299 K To find: Whether the reaction is spontaneous

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A: Given, ΔH° = 24.6 kJ ΔS ° = 132 J/K

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A: Given CO C5H12 H2 Arrange them in order of increasing molar entropy = To be determined

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A: Given  ΔH°= 20 kJ  1 kJ =1000 J ΔH°= 20,000 J ΔS° = 140 J/K T = 298 K  ΔG° = To be determined

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A: Given:

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Q: maximum amount of work

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Q: (Q69) Using the tabulated values from the text (located in Appendix G, beginning at p. 1211)…

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Q: Place the following in order of  increasing molar entropy at 298 K.  CO  ,   C 5H 12 ,    H 2

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Q: How does the entropy of ice at −5°C diff er, if at all, from its entropy at −50°C?

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Q: Under what circumstance can the enthalpy of a system decrease for a spontaneous process?

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Q: Why do exothermic processes tend to be spontaneous at low temperatures?

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Q: Question attached

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Q: For the reaction CO (g) + H,0 «) →C 208) ΔΗ. a) + H. 2(8) · calculate the following reaction's…

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