Trouton\'s rule states that the molar enthalpy of vaporization of a liquid that does not have strong molecular interactions such as hydrogen bonding or ion-ion attractions is given by ΔHvap = (85 J x K^-1 x mol^-1)Tb where Tb is the normal boiling point of the liquid in kelvins.
a) Apply Trouton\'s rule to estimate the value of ΔHvap for these compounds.
Chloromethane, Water, and hydrogen sulfide - all in kJ/mol.

b) Compared to the accepted ΔHvap values (given in the \"Hint\") what is the percentage error in each case?

Question

Trouton\'s rule states that the molar enthalpy of vaporization of a liquid that does not have strong molecular interactions such as hydrogen bonding or ion-ion attractions is given by ΔHvap = (85 J x K^-1 x mol^-1)Tb where Tb is the normal boiling point of the liquid in kelvins. 
a) Apply Trouton\'s rule to estimate the value of ΔHvap for these compounds.   
Chloromethane, Water, and hydrogen sulfide - all in kJ/mol.

b) Compared to the accepted ΔHvap values (given in the \"Hint\") what is the percentage error in each case?