# Sulfur dioxide has a vapor pressure of 462.7 mm Hg at –21.0 °C and a vapor pressure of 140.5 mm Hg at –44.0 °C. What is the enthalpy of vaporization of sulfur dioxide? (R = 8.314 J/K⋅mol)

Answer : The value of is 28.97 kJ/mol

Explanation :

To calculate of the reaction, we use clausius claypron equation, which is:

where,

= vapor pressure at temperature = 462.7 mmHg

= vapor pressure at temperature = 140.5 mmHg

= Enthalpy of vaporization = ?

R = Gas constant = 8.314 J/mol K

= initial temperature =

= final temperature =

Putting values in above equation, we get:

Therefore, the value of is 28.97 kJ/mol

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