o The enthalpy or ∆H of a reaction is defined as the change in energy (more specifically heat energy) for one mole of a substance involved in a process.
It is given that, the enthalpy change for 18g of water (at 100⁰ and 1 bar pressure) is =40.79 kJ mol–1 in the process of vapourisation.
And for water, 18g is =1 mole (For H2O, the calculation of molar mass: 2×1 + 16 = 18g)
Hence, enthalpy change of vapourisation for 1 mole = 40.79 kJ mol–1 enthalpy change of vapourisation for 2 moles of water = (40.79 × 2) = 81.58kJ mol–1
o Standard enthalpy of a process or ∆H⁰ is the enthalpy change of the process when involved substances are in their standard states.
Hence, for water ∆Hvapourisation, ⁰ will be equal to =40.79 kJ mol–1
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