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Intermolecular hydrogen bonding increases the enthalphy of vapourization of a liquid due to the:

(A)decrease in the attraction b/w molecules

(B)increase in the attraction b/w the molecules

(C)decrease in the molar mass of unassociated liquid molecules

(D)increase in the effective molar mass of hydrogen bonded molecules

i did'nt get the meaning of (C) and (D)

ans B D

suchita undare , 14 Years ago
Grade 12th Pass
anser 2 Answers
Aman Bansal

Dear Suchita,

The enthalpy of vaporization, (symbol ΔHvap), also known as the heat of vaporization or heat of evaporation, is the energy required to transform a given quantity of a substance into a gas at a given pressure (often atmospheric pressure).
It is often measured at the normal boiling point of a substance; although tabulated values are usually corrected to 298 , the correction is often smaller than the uncertainty in the measured value.
The heat of vaporization is temperature-dependent, though a constant heat of vaporization can be assumed for small temperature ranges and belowTr<<1.0. The heat of vaporization diminishes with increasing temperature and it vanishes completely at the critical temperature (Tr=1) because above the critical temperature the liquid and vapor phases no longer co-exist.

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Last Activity: 14 Years ago
suchita undare

but what does C and D part mean???

Last Activity: 14 Years ago
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