# Question #c6520

##### 1 Answer

You'd need about **7 times more** energy to vaporize 1 g of water at

Mathematically, you would know this from the difference between water's **latent heat of vaporization** and **latent heat of fusion**.

The *latent heat of fusion* is the heat required to change a substance from solid state to liquid state; likewise, the *latent heat of vaporization* is the heat required to change a substance from liquid state to gas state.

Now, here's why you'd need more energy to go from liquid to vapor than you would to go from solid to liquid.

In ice, water molecules are very closely packed together; the intermolecular forces of attraction are particularly strong in solids, which means that the molecules have little to no freedom to move.

When you heat ice at *still exist*, but the water molecules are no longer stuck in a rigid structure.

When going from liquid to vapor, you must provide sufficient heat so that the kinetic energy of the water molecules overcomes the intermolecular forces altogether, leaving you with molecules that no longer interact with eachother.

This being said, the actual values for the latent heat of vaporization and for the latent heat of fusion for water are

The heat you'd need to supply to **1 gram** of water in each case would be