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.

Ethanol boils at '78.4^circ C'. The enthalpy of vaporisation of ethanol is '42.4 kJmol^(-1)'. Calculate the entropy of vaporisation of ethanol.

If the enthalpy of vaporisation of water is 186.5 kJ mol^(-1) , then entropy of its vaporisation will be

(i) State the second law of thermodynamics ono the basis of entropy. (ii) Boiling point of ethanol is 78.4^(@)C . Change in enthalpy during vaporisation of ethanol is 96J*mol^(-1) , calculate the change in entropy of vaporisation of enthanol.

If the enthalpy of vaporisation of water is 186.5 J mol^(-1) , then entropy of its vaporisation will be

Boiling point of ethanol is 78.4 ^(@) C . Change in enthalpy during vaporisation of ethanol is 96 J * mol^(-1) . Calculate the change in entropy of vaporisation of ethanol .

The enthalpy of vaporisation of water is 186.5 kJ mol^(-1) . The entropy of its vaporisation will be :

Boiling point of an organic compound is 310K . Its enthalpy of vaporisation per mole Delta_(vap)H is 27.9 kJ mol^(-1) . Calculate the entropy of vaporisation Delta_(vap)S of organic compound.