Calculate the enthalpy of vaporisation per mole for ethanol. Given `DeltaS = 109.8 J K^(-1) mol^(-1)` and boiling point of ethanol is `78.5^(@)`.

Calculate the enthalpy of vaporisation per mole for ethanol. Given, ΔS=109.8JK^(−1)mol^(−1) and boiling point of ethanol is 78.5^(@)C .

Calculate the enthalpy of vapourisation of ethanol, given enthalpies of formation of liquid ethanol and gaseous ethanol as -277.6J and -235.4 kJ respectively.

Ethanol boils at 78.4^@C and the enthalpy of vaporisation of ethanol is 42.4kJ mol^(-1) . Calculate the entropy of vaporisation of ethanol.

The value for DeltaH_(vap) and Delta S_(vap) for ethanol are respectively 38.594 kJ mol^(-1) and 109.8 JK^(-1) mol^-1 . The boiling point of ethanol will be

The enthalpy of vaporisation of a substance is 8400 J mol^(-1) and its boiling point is -173^(@)C . The entropy change for vaporisation is :

Calculate the entropy change when 1 mole of ethanol is evaporated at 351 K. The molar heat of vapourisation of ethanol is 39.84 "kJ mol"^(-1)