Chloroform has `DeltaH_("vaporization")=29.2 kJ//"mol"` and boils at `61.2^(@)C`. What is the value of `DeltaH_("vaporization")=29.2 kJ//"mol"` for chloroform ?

Chloroform has DeltaH_("vaporization")=29.2 kJ//"mol" and boils at 61.2^(@)C . What is the value of DeltaS_("vaporization") for chloroform ?

Chloroform has DeltaH_("vaporization")=29.2 kJ//"mol" and boils at 61.2^(@)C . What is the value of Delta S _ ("vaporization") for chloroform ?

Bromine boils at 59^(@)C with DeltaH_(vap)^(@)=29.6kJ mol^(-1) What is the value of DeltaS_(vap)^(@)"in"29.6 J mol^(-1)K^(-1)

The enthalpy of vaporization of chloroform is 29.4 kJmol^(-1) at its normal boiling point of 61.7^(@) C. What is the entropy of condensation of chlorofom at this temperature?

The enthalpy of vaporization of chloroform is 29.4 kJmol^(-1) at its normal boiling point of 61.7^(@) C. What is the entropy of condensation of chlorofom at this temperature?

Calculate Delta E when one mole of liuid is vaporized at its boiling point ( 80^(@)C ) and 1atm pressure . [DeltaH_(vap)=30.7KJ//mol]

The DeltaH for vaporization of a liquid is 20kJ/mol. Assuming ideal behaviour, the change in internal energy for the vaporization of 1 mol of the liquid at 60^(@)C and 1 bar is close to -