Question

1. Define the following:
(a) Specific latent heat of fusion
(b) Specific latent heat of vaporisation,
2. Define the following and state their numerical
value in SI system.
(a) Specific latent heat of fusion of ice.
(b) Specific latent heat of vaporisation of steam.
3. (a) During change of state, temperature does not
rise or fall. What happens to the heat energy
supplied or given out? Explain.
(b) Explain the change of state from solid to liquid
on the basis of kinetic theory.
​

Answer 1

1. Specific latent heat of fusion, lf, of a substance is defined as the amount of heat required to change a unit mass of the substance from solid to liquid state, without any change in the temperature.
2. The specific latent heat of vaporisation of a substance is the quantity of heat required to convert a unit mass of the substance from liquid state to vapour state at its boiling point.

1. While ice melts, it remains at 0 °C (32 °F), and the liquid water that is formed with the latent heat of fusion is also at 0 °C. The heat of fusion for water at 0 °C is approximately 334 joules (79.7 calories) per gram, and the heat of vaporization at 100 °C is about 2,230 joules (533 calories) per gram.
2. A container contains 0. 25 kg of a liquid at its boiling temperature. If the latent heat of fusion for the liquid is 500 Joules/ kg and the latent heat of vaporization for the liquid is 1000 Joules/ Kg.

1. Given in attachment.
2. When a solid is heated, the kinetic energy of the molecules increases. ... When the kinetic energy possessed by the molecules reaches the point where it completely overcomes the intermolecular force, the state changes and the solid turns into a liquid.

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