The heat of fusion of water is larger than the heat of vaporization
No, this statement is incorrect. The heat of vaporization of water is actually larger than the heat of fusion.
The heat of fusion, also known as the enthalpy of fusion, is the amount of heat energy required to change a substance from a solid to a liquid state at its melting point. For water, the heat of fusion is approximately 334 joules per gram.
On the other hand, the heat of vaporization, also known as the enthalpy of vaporization, is the amount of heat energy required to change a substance from a liquid to a gas state at its boiling point. For water, the heat of vaporization is approximately 2260 joules per gram.
Therefore, the heat of vaporization of water is significantly larger than its heat of fusion.
The statement that the heat of fusion of water is larger than the heat of vaporization is incorrect. In reality, the heat of fusion of water is lower than the heat of vaporization.
The heat of fusion of a substance refers to the amount of heat energy required to change one unit of mass from a solid state to a liquid state at its melting point. For water, the heat of fusion is approximately 334 joules per gram (J/g).
On the other hand, the heat of vaporization of a substance refers to the amount of heat energy required to change one unit of mass from a liquid state to a gaseous state at its boiling point. For water, the heat of vaporization is approximately 2260 J/g.
This means that it takes more energy to convert water from a liquid to a gas (vaporize it) than to convert it from a solid to a liquid (fuse it).