Which of the following accounts for the relatively high vapor pressure of diethy

Question

Which of the following accounts for the relatively high vapor pressure of diethyl ether, (CH_3CH_2)O, at 25 degree C? density of the liquid strength of the intermolecular forces strength of the intermolecular forces 1 only 2 only 3 only 1 and 2 only 2 and 3 only Which of the following would be expected to have the highest heat of vaporization? H_2O NH_3 PH_3, AsH_3 SbH_3 The forces of attraction between molecules of are induced dipole-dipole attractions. dipole-dipole attractions. covalent bonds. London forces. dipole-induced dipole attractions. I_2 is a non-polar molecule because each I atom has equal electronegativity towards the bonded electrons such there is no permanent-positive & negative poles between the that bonded atoms. Thus, the only force available to I_2 is London dispersion forces The STRONGEST intermolecular forces between molecules of NH3 are ionic bonds. hydrogen bonds. ion-dipole attractions. London forces. covalent bonds. Note, NH_3, can exhibit hydrogen bonding, dipole-dipole and London force. The order of the strength of intermolecular forces are, ion-dipole, hydrogen bonding, dipole-dipole and London dispersion forces interactions Which of the following molecules exhibits hydrogen bonding? CH_4

Explanation / Answer

The vapor pressure of diethyl ether is reported to be around 0.7 atm at 250 C.

This is because of the intermolecular forces existing between the molecules of diethyl ether. The vapor pressure is relatively high for those compounds which have weak forces. If weak forces are present, the molecules are free to move. Vapor pressure is the tendency of liquid molecules to escape liquid phase and attain gaseous phase. Vapor pressure also depends on temperature. At high temperatures molecules are free to move and have high vapor pressure.

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