Under standard conditions the absolute entropy of liquid water is (H2O(l)) = 69.91 J K-1 mol-1 . What is the change in molar entropy induced by heating the system enough that the resulting vapor has a temperature of 400 K? (Hint – consider the heat capacities to be independent of temperature.)

Q: molar heat capacities for carbon dioxide at 298.0 K are shown below. Cv = 28.95 J K-¹ mol-1 Cp =…

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Q: Consider the reaction 6CO2(g) + 6H2O(l)C6H12O6 + 6O2(g) for which H° = 2.801×103 kJ and S° =…

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Q: The molar heat capacities for carbon dioxide at 298.0 K are shown below. C 28.95 J K-¹ mol-1 C₂ =…

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Q: onsider the reaction 2NaOH(aq) + H2(g)2Na(s) + 2H2O(l) for which H° = 368.6 kJ and S° = 15.30 J/K…

A: Solution- 2NaOH (aq)+ H2O(g)  →2Na(s)+H2O(l)∆Ho= 368.6 kJ ∆S° = 15.30 J/K at 298.15 K.(1). NaOH…

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Q: The heat of fusion AH, of methanol (CH,OH) is 3.16 kJ/mol. Calculate the change in entropy AS when…

A: Heat of fusion of ethanol = 3.16 KJ /molweight of ethanol = 23 gMelting temp. = -98.0 °C…