Question

Melting point, enthalpy of vapourisation and viscosity data of \[\ce{H2O}\] and \[\ce{D2O}\] is given below :

	\[\ce{H, O}\]	\[\ce{D2O}\]
Melting point / K	373.0	374.4
Enthalpy of vapourisation at (373 K)/kJ mol–1	40.66	41.61
Viscosity/centipoise	0.8903	1.107

On the basis of this data explain in which of these liquids intermolecular forces are stronger?

Answer 1

The melting point, enthalpy of vapourisation and viscosity values of all these items depend upon the intermolecular forces of attraction. Since their values are higher for \[\ce{D2O}\] as compared to those of \[\ce{H2O}\], therefore, intermolecular forces of attraction are stronger in \[\ce{D2O}\] than in \[\ce{H2O}\].