## Introduction To Latent Heat Of Water:

In talking about the heats involved in changing temperatures, one thing weâ€™ve neglected is what happens when a material changes phase. We talked about the three phases – gas, liquid, and water. When a material changes from one phase to another, we call this a phase transition or change of phase. Changes from the solid to the liquid or from the liquid to the gaseous state and vice versa are called phase changes.

They always involve a transfer of heat, even though the temperature of the substance undergoing the phase change stays constant. The heat flow from one object to another can change either the average kinetic energy of the random motion of the molecules, which changes the temperature of the object or can change the average potential energy of the molecules, which causes the phase of the object to change. Consider what happens when, for instance, a pot of water is heated on a stove.

At first, the temperature rises. Upon reaching 100Â°C (212Â°F) the temperature stops increasing, even though the flame keeps supplying heat at the same rate as before. We know that the supplied goes into breaking the bonds between the molecules, while the kinetic energy of the molecules remains unchanged. Gradually, more and more molecules gain sufficient energy to overcome the intermolecular forces binding the molecules one to the other. A similar phenomenon occurs when the ice melts.

## What Is Latent Heat?

We call the heat required to produce a phase change the **latent heat** (L’Heat). We can define it as:

Latent heat is energy released or absorbed, by a body or a thermodynamic system, during a constant-temperature process – usually a first-order phase transition.

**Two examples of latent heat are:**

- The heat of freezing
- The heat of vaporization

The heat of freezing is the amount of thermal energy given off as a liquid freezes, and the heat of vaporization is the amount of thermal energy that must be added to change a liquid to a gas.

**You may also want to check out these topics given below!**

- Properties of Water: Anomalous Expansion of Water
- Heat Transfer
- Density Of Water
- Difference Between Heat and Temperature

## Formula Of Latent Heat Of Water

**Heat added or subtracted for a phase change** = Latent heatÂ Ã— Mass

Q = L heat M |

*Where*,

- Q = heat (calories or joules)
- L heat = latent heat (calories/gram or joules/gram)
- M = mass (grams)

### Factors:

- If liquid water at 100Â°C is changed into steam, the heat added (the latent heat of vaporization) is 540 calories for every gram of water.
- If steam at 100Â°C is changed into the water at 100Â° C, 540 calories for every gram of steam must be subtracted. If ice at 0Â°C is changed into liquid water at 0Â°C, the heat added (the latent heat of melting) is 80 calories for every gram of ice.
- If liquid water at 0Â°C changes into ice at 0Â°C, 80 calories for every gram of liquid water must be subtracted.

Latent heats can be very large.

**For example**, the latent heat of vaporization of water is 540 cal/g and the latent heat of freezing of water is 80 cal/g. Therefore, changing a given quantity of water to steam requires 5.4 times as much heat as warming it from 0Â°C (+32Â°F) to 100Â°C (212Â°F), and melting ice requires as much heat as warming water from 20Â°C (68Â°F) to 100Â°C.