Decreasing the temperature reduces the kinetic energy of the gas molecules, allowing them to come closer together. Increasing the pressure forces the molecules closer together, overcoming their natural tendency to spread out.
Here's why:
* Low Temperature: At high temperatures, gas molecules have a lot of kinetic energy and move rapidly, making it difficult for them to condense. Lowering the temperature reduces their kinetic energy, causing them to move slower and collide less frequently. This allows intermolecular forces to take effect, attracting the molecules together.
* High Pressure: Increasing the pressure forces the gas molecules closer together, reducing the space between them. This increased proximity allows intermolecular forces to become more significant, again contributing to the condensation process.
In essence, low temperature and high pressure work synergistically to reduce the kinetic energy of the molecules and increase the likelihood of them forming intermolecular bonds, leading to liquefaction.
