Explain, in terms of the behaviour of water molecules, why there is a difference in the energy required for heating water to its boiling point and changing the same amount of boili... Explain, in terms of the behaviour of water molecules, why there is a difference in the energy required for heating water to its boiling point and changing the same amount of boiling water into steam at 100 °C.
Understand the Problem
The question is asking to explain why heating water to its boiling point requires less energy compared to the energy required to change boiling water into steam. This involves discussing the behavior of water molecules during both processes.
Answer
More energy is needed to break hydrogen bonds for vaporization than to heat water to 100°C.
The difference in energy is due to the need to overcome hydrogen bonds between water molecules. Heating water to its boiling point increases kinetic energy, but vaporizing it requires breaking these strong intermolecular forces, which requires significantly more energy.
Answer for screen readers
The difference in energy is due to the need to overcome hydrogen bonds between water molecules. Heating water to its boiling point increases kinetic energy, but vaporizing it requires breaking these strong intermolecular forces, which requires significantly more energy.
More Information
Vaporization requires overcoming intermolecular hydrogen bonds, which is a higher energy process than merely increasing the temperature.
Tips
A common mistake is confusing the energy needed for temperature change with energy needed for phase change.
Sources
- Why does the temperature of boiling water remain the same... - Vaia - vaia.com
- Steam vs. Boiling Water - Chemistry Community - lavelle.chem.ucla.edu
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