how is the enthalpy of vaporization related to intermolecular forces during a phase change?\na the…

how is the enthalpy of vaporization related to intermolecular forces during a phase change?\na the temperature increase converts bonding forces into intermolecular forces during vaporization.\nb the intermolecular energy of vaporization represents a greater change increasing the bonding forces.\nc the kinetic energy of the ethanol molecules increases strength of the intermolecular forces increases.\nd the liquid state is stabilized by the molecules intermolecular forces resulting in a high enthalpy of vaporization.

how is the enthalpy of vaporization related to intermolecular forces during a phase change?\na the temperature increase converts bonding forces into intermolecular forces during vaporization.\nb the intermolecular energy of vaporization represents a greater change increasing the bonding forces.\nc the kinetic energy of the ethanol molecules increases strength of the intermolecular forces increases.\nd the liquid state is stabilized by the molecules intermolecular forces resulting in a high enthalpy of vaporization.

Answer

Brief Explanations:

The enthalpy of vaporization is the energy required to change a liquid to a gas. Stronger intermolecular forces hold molecules in the liquid - state more tightly. More energy (higher enthalpy of vaporization) is needed to overcome these forces and vaporize the substance. So, the liquid state being stabilized by intermolecular forces leads to a high enthalpy of vaporization.

Answer:

D. The liquid state is stabilized by the molecule's intermolecular forces resulting in a high enthalpy of vaporization.