Following is the - complete Answer -&- Explanation: for the given: Question: in....typed format....
Answer:
Explanation:
Following is the complete Explanation: for the above: Answer.
We are given with the following: information:
compound | chemical formula | Theoritical heat of vaporization; Hvap | Boiling point, Tb , Kelvin ( K ) |
chloromethane | CH3Cl | Hvap = 21.40 kJ/mol | Tb = 249.06 K ( Kelvin ) |
Water | H2O | Hvap = 40.65 kJ/mol | Tb = 373.15 K ( Kelvin ) |
Hydrogen sulfide | H2S | Hvap = 18.67 kJ/mol | Tb = 213.6 K ( Kelvin ) |
We know that: according to Trouton's rule: the following:
Calculated: Hvap = ( 85.0 J / K. mol ) x ( Tb ) -------------------------Equation - 1
Using the given: information: and Equation - 1; we can form the following table: using MS Excel: presented below, in image format....
We know: we can calculate, the percent errors: in the above calculations, for each of the compounds using the following: formula:
i.e. percent error = { [ calculated Hvap - Theoritical Hvap ] / ( Theoritical Hvap) } x 100.0 % --- Equation - 2
Using the above information and Equation - 2: and using MS Excel: we get the following: table: in....image format...
Trouton's rule states that the molar enthalpy of vaporization of a liquid that does not have...
2. A useful generalization known as the Trouton's rule states that, for many non-associated liquids at their normal boiling point, the standard molar entropy of vaporization has a value of about 87 J molK. a) Given that the standard molar enthalpy of vaporization for water is 40.7 kJ mol , calculate the standard molar entropy of vaporization of water. b) Does water obey Trouton's rule? Explain. c) The normal boiling point of CC2F2 is -29.79 °C and AH ap 20.2...