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Chapter 10: Q10.3-46 E (page 588)

Explain why the enthalpies of vaporization of the following substances increase in the order CH4 < NH3 < H2O, even though all three substances have approximately the same molar mass.

Short Answer

Expert verified

The greater the intermolecular forces of attraction, greater will be the enthalpies of vaporization.

Step by step solution

01

The concept

The greater the intermolecular forces of attraction, the greater the vaporization's enthalpies. Order of strength of intermolecular forces: - Hydrogen bonding > Dipole-Dipole > Weak dispersion force (London Force).

Methane (CH4) is a nonpolar molecule, whereas ammonia (NH3) and water (H2O) are polar molecules. Therefore, methane will experience a weak dispersion force, and thereby it will have the lowest enthalpy of evaporation.

02

To explain why the enthalpies of vaporization increases

Now, both ammonia and water are capable of forming hydrogen bonds. Still, since the polarity O-H bond is more than the polarity of the N-H bond, therefore water will form a stronger hydrogen bond as compared to ammonia. Therefore, the water will have a greater enthalpy of evaporation than ammonia.

Hence, the greater the intermolecular forces of attraction, the greater the vaporization's enthalpies.

Order of strength of intermolecular forces: - Hydrogen bonding > Dipole-Dipole > Weak dispersion force (London Force).

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