At 0°C and 100°C, water undergoes phase transitions (freezing and boiling, respectively), and the energy input is absorbed or released as latent heat, temporarily halting temperature change.
The phenomenon of temperature stabilization at 0°C and 100°C is attributed to the phase transitions of water. At 0°C, water undergoes the process of freezing, transitioning from a liquid to a solid state. During this phase transition, energy is absorbed as latent heat to break the intermolecular bonds and convert the liquid into a solid. Similarly, at 100°C, water transitions from a liquid to a gaseous state through the process of boiling.
The absorption of energy occurs as water molecules overcome attractive forces and transform into vapor. The absorbed or released energy during these phase transitions temporarily halts any change in temperature, resulting in a plateau in the temperature-time graph until the entire substance undergoes the phase transition. This behavior is a characteristic property of water and is crucial in processes such as heating or cooling substances involving water.