Calculate the Standard Molar Entropy of methanol ( CH3OH) and ethanol ( C2H5OH) at 25 celcius...

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Chemistry

Calculate the Standard Molar Entropy of methanol ( CH3OH) andethanol ( C2H5OH) at 25 celcius or 298.15 K. Once calculatedexplain WHY one has a high standard molar entropy.
Given = melting point of methanol is 175.47 K; enthaply offusion is 3.18 KJ/mol; boiling point is 337.7K; enthalpy ofvaporization is 35.21 KJ/mol
melting point of ethanol is 159.0K; enthalpy of fusion is5.02KJ/mol; boiling point is 351.44 K; and enthalpy of vaporizationis 38.56 KJ/mol
. . . . so I dont know what equations I can use given theseknowns but here are some potential equations to use:
Gm(standard) = Hm(standard) - TSm(standard) . . . . m is molarso Gm= G / mol
Delta S of Vaporization = delta H vaporization / T
Delta S fusion = delta H fusion / T
I am supposed to be able to do the problem with only the GIVENinformation so hopefully someone can help me! Thanks and I willrate.

Answer & Explanation Solved by verified expert

4.3 Ratings (740 Votes)

To calculate the S0 you need to calculate the entropy from 0 Kto 298 K in the following orderS from the heat capacity 0KTemperature of fusion S from the change of state fusion See Answer

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