The temperature remains constant during a phase transition because energy is being absorbed or released by the substance as it changes from one phase to another. This energy is used to break or form intermolecular bonds, rather than increasing the temperature.
The temperature at which a phase transition occurs is determined by the strength of intermolecular forces in the substance, as well as external factors such as pressure and the presence of impurities.
Yes, the temperature at which a phase transition occurs can be changed by altering external factors such as pressure or the presence of impurities. However, the strength of intermolecular forces in the substance will ultimately determine the temperature range over which the phase transition can occur.
Some substances have multiple phase transitions at different temperatures because they may have different phases with different intermolecular forces. These different phases will transition at different temperatures depending on the strength of their respective intermolecular forces.
No, the temperature is not always constant during a phase transition. In some cases, a substance may absorb or release enough energy to cause a change in temperature during a phase transition. This is known as a latent heat of fusion or vaporization, and can be observed in substances like water during the phase transitions between solid, liquid, and gas.