The heat of vaporization ΔΗν of tetrahydrofuran (C4H80) is 32.0 kJ/mol. Calculate the change in entropy AS when 8.2 g of tetrahydrofuran boils at 66.0 °C Be sure your answer contains a unit symbol and the correct number of significant digits.

The entropy change of the tetrahydrofuran is 70.8 J/K

Explanation:

To calculate the number of moles, we use the equation:

Given mass of tetrahydrofuran = 8.2 g

Molar mass of tetrahydrofuran = 72 g/mol

Putting values in above equation, we get:

To calculate the entropy change for different phase at same temperature, we use the equation:

where,  

= Entropy change  = ?

n = moles of tetrahydrofuran = 0.114 moles

= enthalpy of vaporization = 32.0 kJ/mol = 32000 J/mol   (Conversion factor:  1 kJ = 1000 J)

T = temperature of the system =

Putting values in above equation, we get:

Hence, the entropy change of the tetrahydrofuran is 70.8 J/K

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