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The enthalpy of vaporization of methanol is 35.27 kJ/ mol at 64.1 oC. Determine the entropy...

The enthalpy of vaporization of methanol is 35.27 kJ/ mol at 64.1 oC. Determine the entropy change in the system for the vaporization of 2.00 moles of methanol. What is the entropy change in the surroundings (assume Tsurr = 25 oC.)

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Answer #1

1)as we know

S= vapH / Tb= 35.27 / 337.1 = 0.10463 kJ/ mol K T= 64.10C= 337.1 K

2)

S= system + surrounding = ( as vapourisation is assumed reversible then

0=  system + surrounding

surrounding = - 0.10463 kJ/ mol K  

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