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Chapter 12: Problem 20

Explain why vaporization occurs only at the surface of a liquid until the boiling point temperature is reached. That is, why does vapor not form throughout the liquid at all temperatures?

Short Answer

Expert verified
Vaporization typically occurs only at the surface of a liquid because surface molecules lack other liquid molecules on all sides, and hence are subjected to fewer intermolecular forces. Once the temperature reaches the boiling point, vapor can form throughout the liquid as the vapor pressure equals the atmospheric pressure, allowing the energy provided to overcome the intermolecular attractions.

Step by step solution

01

Definition of Vaporization

Vaporization is the transition process from a liquid phase to a gaseous phase. It can happen in two ways: evaporation or boiling. Evaporation is a surface phenomenon, while boiling occurs throughout the liquid.
02

Understanding Surface Phenomena

The molecules at the surface of the liquid do not have other liquid molecules on all sides, which leads to fewer intermolecular forces acting on them. Therefore, these surface molecules require a lesser amount of energy to overcome these forces and escape as vapor.
03

Role of Temperature

When the temperature of the liquid is less than the boiling point, only the surface molecules possess the necessary energy to turn into vapor. Therefore, vaporization only occurs at the surface of the liquid at temperatures below the boiling point.
04

Understanding the Boiling Point

When the temperature reaches the boiling point, the vapor pressure is equal to the atmospheric pressure. At this point, the energy provided is sufficient for the molecules inside the liquid to overcome the intermolecular attraction and become vapor. Hence, vapor forms throughout the liquid at the boiling point.

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