Answer:
a. CH4 is only held together by London dispersion forces since any dipoles cancel out due to symmetry. On the other hand H2O has strong hydrogen bonds
b. PH3 has dipole-dipole forces while NH3 is held together by stronger hydrogen bonding
c. C2H6 and C3H8 . Both substances are held together by London dispersion forces since any dipoles cancel out due to symmetry. However C3H8 has the stronger London dispersion forces of the two because it is a larger molecule,
d. BH3 is held together by London dispersion forces since any dipoles cancel out due to symmetry while OF2 is held together by stronger dipole-dipole forces
The water has more standard enthalpy of vaporization than methane. [tex]\bold {\Delta V_{vap}}[/tex] is required to vaporize a mole of substance.
It is the amount of energy that is required to vaporize a mole of substance. It is mainly depends up on inter molecular bonds.
The inter-molecular bond in Methane is only London dispersion forces while the water molecules are held together by hydrogen bonds. Thus the water has more [tex]\bold {\Delta V_{vap}}[/tex].
Therefore, the water has more standard enthalpy of vaporization than methane.
Learn more about inter-molecular bonds.
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