As a substance is heated from its liquid phase to its gas phase, what happens to the spacing and speed of its molecules?
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Spacing and speed increase.
As a substance transitions from its liquid phase to its gas phase, both the spacing and speed of its molecules change. Let me explain how and why this happens.
First, when a substance is in its liquid phase, the molecules are close together and have relatively low kinetic energy. The intermolecular forces between the molecules, such as hydrogen bonding or van der Waals forces, are strong enough to keep them condensed and in a fixed position.
However, when heat is added to the substance, its temperature increases. As the temperature rises, the average kinetic energy of the molecules also increases. This increase in kinetic energy enables the molecules to overcome the intermolecular forces and move more freely.
The increased kinetic energy leads to an increase in the spacing between the molecules. As the molecules gain more energy, they move apart from each other, resulting in a larger average distance between them. This expansion of the substance leads to a change from the liquid phase to the gas phase.
Additionally, the increase in kinetic energy also affects the speed of the molecules. The individual molecules gain more energy and, as a result, move faster. This increase in molecular speed is directly related to the rise in temperature.
In summary, the spacing between molecules increases as they transition from the liquid phase to the gas phase due to the increased kinetic energy. Simultaneously, the individual molecules move faster as their kinetic energy rises, resulting in the change of state from liquid to gas.