Sarath is heating water in a closed container. He wants to boil the water. But he is wondering whether the water will boil or not. Can you help him? Will water boil in that closed container?
Sarath is heating water in a closed container. He wants to boil the water. But he is wondering whether the water will boil or not. Can you help him? Will water boil in that closed container?
The correct option is B No
For this, first we need to know what is boiling.
Boiling is a special case of evaporation. It is the rapid conversion of a liquid into vapour by means of formation of bubbles. During boiling, vaporization is not restricted to the surface only but takes place throughout the bulk of the liquid.
The condition of free vaporization throughout the liquid is called boiling.
The temperature at which the vapour pressure of a liquid is equal to the external pressure is called the boiling temperature at that pressure. At 1 atm pressure, the boiling temperature is called boiling temperature is called normal boiling point. If the pressure is bar, then the boiling point is called standard boiling point of the liquid.
Now, what happens if we do this in a closed vessel?
Boiling does not occur when a liquid is heated in a closed vessel. On heating continuously, vapour pressure increases. At first a clear boundary is visible between liquid and vapour phases because the liquid is denser than vapour. As the temperature increases, more and more molecules go into vapour phase and the density of vapour rises. At the same time, the liquid becomes less dense. It expands because molecules move apart. When the densities of the liquid and vapours become same, the clear boundary between them disappears. This temperature is called critical temperature.
For this, first we need to know what is boiling.
Boiling is a special case of evaporation. It is the rapid conversion of a liquid into vapour by means of formation of bubbles. During boiling, vaporization is not restricted to the surface only but takes place throughout the bulk of the liquid.
The condition of free vaporization throughout the liquid is called boiling.
The temperature at which the vapour pressure of a liquid is equal to the external pressure is called the boiling temperature at that pressure. At 1 atm pressure, the boiling temperature is called boiling temperature is called normal boiling point. If the pressure is bar, then the boiling point is called standard boiling point of the liquid.
Now, what happens if we do this in a closed vessel?
Boiling does not occur when a liquid is heated in a closed vessel. On heating continuously, vapour pressure increases. At first a clear boundary is visible between liquid and vapour phases because the liquid is denser than vapour. As the temperature increases, more and more molecules go into vapour phase and the density of vapour rises. At the same time, the liquid becomes less dense. It expands because molecules move apart. When the densities of the liquid and vapours become same, the clear boundary between them disappears. This temperature is called critical temperature.
