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When a phase change is occurring the temperature of the sample stays the same because the heat that is being added to the sample is being used to break the bonds of the sample instead of raise the temperature. For example, if we have ice that has reached its freezing point, the heat that is being applied to it is now being used to break the bonds in the ice. When the phase change is complete and ice has turned completely into water, then the temperature will begin to rise again until water reaches its boiling point and begins to turn into steam.
Temperature is typically constant when heat is added to a substance that is undergoing a phase change. Heat energy is stored as potential energy that is used to break the molecular bonds. For example, in ice, as heat is applied at 0 degrees Celsius, the temperature stays constant until the ice has undergone the phase change into water. The heat energy is converted into potential energy that allows the water molecules to spread apart and move loosely between each other.
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