Melting point,enthalpy of vaporisation and viscosity data of $H_2O$ and $D_2O$ is given below.
$Property$ $H_2O$ vs $D_2O$ $Melting$ $point/K$ $273.0$ vs $276.8$ $Enthalpy$ $of$ $vaporisation$ $at$ $(373 \ K) / kJ \ mol^{-1}$ $40.66$ vs $41.61$ $Viscosity/centipoise$ $0.8903$ vs $1.107$
On the basis of this data,explain in which of these liquids intermolecular forces are stronger?
| $Property$ | $H_2O$ vs $D_2O$ |
| $Melting$ $point/K$ | $273.0$ vs $276.8$ |
| $Enthalpy$ $of$ $vaporisation$ $at$ $(373 \ K) / kJ \ mol^{-1}$ | $40.66$ vs $41.61$ |
| $Viscosity/centipoise$ | $0.8903$ vs $1.107$ |
On the basis of this data,explain in which of these liquids intermolecular forces are stronger?
(N/A) The melting point,enthalpy of vaporization,and viscosity are physical properties that depend on the magnitude of intermolecular forces of attraction.
As observed from the data,the values for $D_2O$ are consistently higher than those for $H_2O$.
This indicates that the intermolecular forces of attraction (specifically hydrogen bonding) are stronger in $D_2O$ compared to $H_2O$.
As observed from the data,the values for $D_2O$ are consistently higher than those for $H_2O$.
This indicates that the intermolecular forces of attraction (specifically hydrogen bonding) are stronger in $D_2O$ compared to $H_2O$.
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