In this article we will be discussing about, latent heat of water, specific latent heat of vaporization of water, latent heat of vaporization of water, how to increase the latent heat of vaporization, what is the latent heat vaporization value, latent heat of ice in calories, latent heat of water in calories, latent heat of steam in calories, example of latent heat.
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Latent heat is defined as a heat which is emitted or absorbed by a substance during the change of phase and without a temperature change. Here the phase change is transition of liquid to solid or gas, transition of solid to liquid or gas, transition of gas to solid or liquid. Generally latent heat is represented in joules or calories in unit mass.
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As mentioned before latent heat is heat required for phase change without temperature change. Similarly, latent heat of water is heat required for phase change of water without change in temperature of water. Here phase change is transition of water to ice or vapor, ice to water or vapor. When there is transition of state from liquid to solid and gas to liquid, during that time heat will be released (exothermic). When there is transition of state from liquid to gas and solid to liquid, during that time heat will be absorbed (endothermic).
Generally latent heat of water is of two types:
Formula to calculate latent heat
L=Q/M
Were Q is the heat quantity
M is the body mass
L is latent heat
This equation states that the amount of heat released or absorbed by the substance of mass M gives as latent heat. The latent heat unit is given by J/Kg
Also read :
Latent heat of fusion:
Latent heat of fusion refers to melting a solid and freezing a liquid without change in temperature. Here melting a solid, means melt a ice (transition of solid phase to liquid phase) and freezing a liquid means cools down a liquid to ice (transition of liquid phase to solid phase)
Example of latent heat of fusion (1 calorie = 4.186 J)
Consider 1kg of ice at zero-degree Celsius, the amount of heat required to melt the ice to water is latent heat of fusion of 1kg of water is equal to 79.5 Cal/g or 333.55 kJ/kg without change in temperature. Similarly, the reverse effect of this is solidification i.e. the amount of heat required for freezing the water to ice is the same as heat required to melt the ice to water but with negative sign. So, the energy radiated by water to become ice is the same as energy absorbed by ice to become water.
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Latent heat of vaporization of water:
Latent heat of vaporization refers to boiling a liquid and condensing a gas without change in temperature. Here boiling a liquid means we are going to heat the water (transition of liquid phase to gas phase) and condensing a gas means we are going to cool or condense the evaporated water (transition of gas phase to liquid phase).
Example of latent heat of vaporization of water
Consider a bucket of water boiling at 100-degree Celsius, the amount of energy required to change water to vapor is 540 Cal/g. Similarly, the energy required to condense the vapor back to water is -540cal/g. So, the latent heat of vaporization of water is 2257 kJ/kg.
NCERT Physics Notes:
Specific latent heat
Specific latent heat is defined as the amount of heat required for transition of one phase completely to another phase for a unit mass. The heat capacity of a particular substance depends upon the mass of that substance. But the specific heat capacity (s) does not depend on the mass of the substance. Specific heat capacity is defined as at constant pressure the amount of heat required to increase the temperature to 1-degree Celsius for 1gram of substance. Specific latent heat is represented in J/Kg. This can be given as to increase the temperature to 1-degree Celsius for 1gram of water, we require 4.186J of heat or 1calorie. To calculate the heat required for change in temperature we can use this equation
q=m×s×∆t
Were q is heat required
m is mass of substance
s is specific heat
∆t change in temperature
This equation cannot be used when transition of phase takes place. For example, transition from solid, liquid and gas phase. Because when the heat is increased or decreased it does not cause change in temperature.
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Latent heat is defined as a heat which is emitted or absorbed by a substance during the change of phase but without a temperature change. It is calculated by
L=Q/M
Were Q is the heat quantity
M is the body mass
L is latent heat
The unit for latent heat is J/Kg
Specific heat is defined as the change in temperature of substance but without change in phase like solid to liquid or vice versa. It is calculated by
q=m×s×∆t
Were q is heat required
m is mass of substance
s is specific heat
∆t change in temperature
The unit for specific heat is J/Kg. K
The latent heat of water is heat required for phase change of water without change in temperature of water. When there is transition of state from liquid to solid and gas to liquid, during that time heat will be released (exothermic). When there is transition of state from liquid to gas and solid to liquid, during that time heat will be absorbed (endothermic).
generally latent heat of water is of two types
latent heat of fusion
latent heat of vaporization
Formula to calculate latent heat
L=Q/M
Were Q is the heat quantity
M is the body mass
This equation states that the amount of heat released or absorbed by the substance of mass M gives as latent heat. The latent heat unit is given by J/Kg
1 calorie = 4.186 J
The latent heat of vaporization of the stream is 540 Cal/g. In SI unit 2257 kJ/kg.
The latent heat of vaporization of the stream is 79.5 Cal/g. In SI unit 333.55 kJ/kg.
Specific heat is defined as the change in temperature of substance but without change in phase like solid to liquid or vice versa. It is calculated by
q=m×s×∆t
Were q is heat required
m = 50g
s is specific heat
∆t change in temperature = 100℃ - 30℃
= 70℃
q=m×s×∆t
q=50×s×70
The heat emitted by a stream can be calculated by latent heat. Because the condensation process is happening during this heat will be released.
L=Q/M
Were Q is the heat quantity
M is the body mass
Q=M*L
Q=1*600
Q=600cal
Heat absorbed = heat released
50×s×70=600
3500*s=600
s=0.17 cal/g ℃
Decreases
The boiling point of water increases when we increase the pressure, so to break the bond of water molecular force only a small amount of energy is required. So only the latent heat of the stream will be decreased when we increase the pressure.
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