In a liquid, the molecules are quite close together so that there are considerable forces of attraction between them and hence they are held together in a definite volume.
The liquids possess fluidity like gases but incompressibility like solid.
Properties of liquid
1)Liquids have no definite shape: They take up the shape of the vessel in which they are put. This is because the molecules in a liquid are in a state of constant rapid motion.
2)liquids have a definite volume: This is because the intermolecular forces of attraction in a liquid are quite strong and unlike gas molecules, the liquid molecules are not completely free to move.
3)liquids have much higher density than gases:This is because the molecules in a liquid are quiet close together. Thus the molecules are much more closely packed than those of the gases.
4)Compressibility :liquids are much less compressible than gases.This is because the intermolecular distances of separation are much smaller in liquid than that in gases.
5)Diffusion: liquids diffuse like gases but the diffusion is much slower because the liquid molecules are quite close, they undergo a much larger number of collisions with each other.
Suppose some liquid is placed in an evacuated vessel connected to a manometer. According to kinetic theory of liquids, the molecules of the liquid are constantly moving in different directions with different speeds. As these molecules are moving with different speeds, they possess different kinetic energy.
At any particular temperature ,the energy of some of the molecules may be so high that they may overcome the forces of attraction by the neighbouring molecules and may leave the liquid and come in the space above the liquid. This process is called evaporation
As the time passes, more and more molecules of the liquid leave the liquid and come in space above the liquid. The molecules thus present above the liquid are called vapour. The molecules in the vapour phase are also constantly moving and some of them strike the surface of the liquid and maybe recaptured by the liquid. The process is called condensation.
If the liquid is added into the evacuated vessel ,then initially, as there are no molecules of vapour, the rate of condensation is zero.
If the temperature is kept constant, the evaporation continues at constant rate as shown by the straight line plot. With the passage of time ,as a number of molecules in the vapour phase becomes more and more ,the rate of condensation also increases.
A stage is reached when rate of condensation becomes equal to rate of evaporation i.e. as many molecules re-enter into a liquid as leave the liquid in the same time.This state is called state of equilibrium .
The pressure exerted by the vapours at this stage is called vapour pressure or saturated vapour pressure as the vapour phase is saturated with vapours at this stage.
Vapour pressure of a liquid at any temperature may be defined as the pressure exerted by the vapour present above the liquid in equilibrium with the liquid at that temperature.
Important results related with process of evaporation
1)Cooling caused by evaporation
When a liquid evaporates ,the more energetic molecules leave the liquid. As a result the average kinetic energy of the remaining liquid decreases and hence the temperature falls.
2)Factors affecting vapour pressure
1)Nature of the liquid : If the intermolecular forces of attraction in the liquid are weak ,the molecules can easily leave the liquid and come into vapour phase and hence the vapour pressure is higher.
For ex: The vapour pressure of acetone, benzene is higher than that of water at same temperature.
2)Effect of temperature: As the temperature of a liquid is increased, the vapour pressure of liquid increases.
3)Boiling point : The vapour pressure of a liquid increases as the temperature is increased. The vapour escaping are only from the surface of the liquid. If the temperature is further increased till the vapour pressure becomes equal to atmospheric pressure, the vapour in the form of bubbles from below the surface start rising to the surface and escape into the air. The temperature at which this happens is called boiling point.
Boiling point of a liquid is defined as the temperature at which the vapour pressure of the liquid becomes equals to external pressure.
When the external pressure is normal atmospheric pressure, the boiling point is called normal boiling point.
When the external pressure is equal to 1 bar, the boiling point is called standard boiling point of the liquid.
Standard boiling point of a liquid is slightly less than the normal boiling point because one bar is slightly less than 1 atmosphere pressure.
Application of effect of external pressure on boiling point
1) If the external pressure is higher, more heat will be required to make the vapour pressure equal to external pressure and hence higher will be the boiling point. That is why in hospitals ,the surgical instruments are sterilised in autoclaves in which boiling point of water is raised by using a weigh to cover the vent.
2)If the external pressure is decreased, the boiling point is lowered. This is the reason that a liquid boils at a lower temperature on the top of the mountain than on the sea shore.That is why at hills, use of pressure cooker is essential for cooking food.
3)It is used for purifying the unstable liquids by distillation under reduced pressure.
4)Heat of vaporisation:
When the liquid starts boiling ,if extra heat is supplied to the liquid, it is used up not in increasing the temperature of the liquid but to overcome the intermolecular forces of attraction, existing in the liquid and thus changing the liquid into vapour. Hence the temperature remain constant till whole of the liquid changes into vapour.
The amount of heat required to change 1 mole of the liquid into its vapour at the boiling point is called the heat of vaporisation of the liquid.
Greater the intermolecular forces of attraction present in a liquid, greater is the heat of vaporisation and higher is the boiling point.