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प्रश्न
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?
उत्तर
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 \[\ce{H2O}\].
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