Changing the internal energy of a material will cause it to change temperature or change state:
As there are two boundaries, solid/liquid and liquid/gas, each material has two specific latent heats:
Some typical values for specific latent heat include:
|Substance||Specific latent heat of fusion (kJ/kg)||Specific latent heat of vaporisation (kJ/kg)|
An input of 334,000 joules (J) of energy is needed to change 1 kg of ice into 1 kg of water. The same amount of energy needs to be taken out of the liquid to freeze it.
The amount of thermal energy stored or released as the temperature of a system changes can be calculated using the equation:
energy required for a change of state = mass × specific latent heat
This is when:
How much energy is needed to freeze 500 grams (g) of water from 0°C?
= 0.5 × 334,000
= 167,000 J
Latent heat can be measured from a heating or cooling curve line graph. If a heater of known power is used, such as a 60 W immersion heater that provides 60 J/s, the temperature of a known mass of ice can be monitored each second. This will generate a graph that looks like this.
The graph is horizontal at two places. These are the places where the energy is not being used to increase the speed of the particles, increasing temperature, but is being used to break the bonds between the particles to change the state.
The longer the horizontal line, the more energy has been used to cause the change of state. The amount of energy represented by these horizontal lines relates to the latent heat.
If a horizontal line that shows boiling on a heating curve is 1 hour 3 minutes long, how much energy has a 60 watt (W) heater provided to the water?
63 minutes = 3,780 s
60 W means 60 J of energy is supplied every second
energy = power × time
energy = 60 × 3,780
energy = 226,800 J
If this energy had caused 100 g of water to evaporate, what is the latent heat of vaporisation of water?
226,800 J for 100 g is equivalent to 2,268,000 J for 1 kg.
The latent heat of vaporisation of water is 2,268,000 J/kg.