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The Kinetic Molecular Theory (KMT) is fundamental in understanding the behavior of particles in different states of matter. It particularly sheds light on how particles move and interact with each other.

According to KMT, particles such as atoms and molecules are always in motion, with gases displaying the most energetic particles of the three common states of matter (solid, liquid, and gas). The theory posits that particles in a gas are in constant, random motion, moving in straight lines until they collide with something else, like another particle or the walls of a container. These collisions are elastic, meaning they don't lose energy in the process, which is a crucial point when considering the behavior of gases.

The theory also explains that the spaces between gas particles are much larger than the particles themselves, which is why gases can be compressed more than liquids or solids. Lastly, the average kinetic energy of these particles is directly related to temperature—a higher temperature means higher kinetic energy and vice versa. This is essential in understanding how temperature affects the phase of a substance—the basis for understanding the process of condensation.

Matter exists in various forms, more commonly known as states. The three principal states are solid, liquid, and gas. In a solid, atoms or molecules are closely packed in a regular arrangement and merely vibrate about fixed positions. They possess the least amount of kinetic energy compared to the other states.

In contrast, liquids have a definite volume but take the shape of their container, with particles that are still close together but can move past one another. This gives liquids a fixed volume but not a fixed shape. Finally, gases have neither a fixed volume nor shape, readily expanding to fill the shape and volume of their container. Here, the particles are far apart and move freely at high speeds, signifying high kinetic energy.

These states of matter can transition from one to another through processes called phase changes. Understanding these states and their properties is crucial in comprehending how substances interact and change under different conditions, as characterized by the Kinetic Molecular Theory.

A phase change is a transition of matter from one state to another, such as solid to liquid (melting), liquid to gas (evaporation), gas to liquid (condensation), or liquid to solid (freezing). During a phase change, the actual temperature of the substance remains constant while the particles absorb or release energy.

When we talk about condensation, we refer to the process where vapor (gaseous water) turns into liquid. Condensation is not just a cooling process but also a reduction in average kinetic energy. As per KMT, when the vapor cools, the average kinetic energy of its particles decreases. When it's energetic enough, a particle resists the cohesive forces trying to bind it; but as it loses energy, it moves more slowly, and these forces pull it into a more closely packed arrangement characteristic of a liquid.

Moreover, pressure also plays a vital role. Increased pressure pushes particles closer together, facilitating a phase change if the temperature and the nature of the substance are conducive to a change in state. In cooling the average kinetic energy and under the right pressure, numerous vapor particles will lose energy, merge, and form a liquid—this is condensation, a critical concept not just in the lab but in everyday phenomena such as dew formation on grass or fog on a windowpane.