Standard enthalpy of vapourisation `Delta_(vap) H^-` for water at 100° C is 44.66 `kJmol^(–1)`. The internal energy of vapourisation of water at 100°C (in `kJmol^(–1)`) is ?

Explanation

To find the internal energy of vaporization of water at 100°C, we can use the relationship between the standard enthalpy of vaporization (ΔH_vap) and the internal energy of vaporization (ΔU_vap). The equation that relates these two quantities is:

\[ \Delta H_{vap} = \Delta U_{vap} + \Delta N_g RT \]

Where:
- ΔH_vap is the standard enthalpy of vaporization.
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