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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

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

Grade:12th Pass

2 Answers

Aman Bansal
592 Points
10 years ago

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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suchita undare
20 Points
9 years ago

but what does C and D part mean???

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