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The Ice House. Tim Clare. Canongate Books , 2 Mei - halaman. War doesn't end. It sleeps. Delphine Venner is an old woman now. She is old, but she remembers everything. She remembers what it is to be a child of war, she remembers fighting for her life and she remembers what the terrifying creatures from another world took from her all those years ago. She remembers the gateway, and those she lost. This macroscopic behavior demonstrates quite clearly that energy must be supplied to a solid in order to melt it.

On a microscopic level melting involves separating molecules which attract each other. This requires an increase in the kinetic energy of the molecules, and the necessary energy is supplied by the heating coil. Selected molar enthalpies of fusion are tabulated below.

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Solids like ice which have strong intermolecular forces have much higher values than those like CH 4 with weak ones. When a liquid is boiled, the variation of temperature with the heat energy supplied is similar to that found for melting.


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When heat is supplied at a steady rate to a liquid at atmospheric pressure, the temperature rises until the boiling point is attained. After this the temperature remains constant until the enthalpy of vaporization has been supplied. Once all the liquid has been converted to vapor, the temperature again rises. In the case of water the molar enthalpy of vaporization is In other words. Heat energy is absorbed when a liquid boils because molecules which are held together by mutual attraction in the liquid are jostled free of each other as the gas is formed.

Such a separation requires energy.


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In general the energy needed differs from one liquid to another depending on the magnitude of the intermolecular forces. We can thus expect liquids with strong intermolecular forces to have larger enthalpies of vaporization. The list of enthalpies of vaporization given in the table bears this out.

Two other features of the table deserve mention. One is the fact that the enthalpy of vaporization of a substance is always higher than its enthalpy of fusion. When a solid melts, the molecules are not separated from each other to nearly the same extent as when a liquid boils. Second, there is a close correlation between the enthalpy of vaporization and the boiling point measured on the thermodynamic scale of temperature. Periodic trends in boiling point closely follow periodic trends in heat of vaporization.


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  7. If we divide the one by the other, we find that the result is often in the range of 75 to 90 J K —1 mol —1. To a first approximation therefore the enthalpy of vaporization of a liquid is proportional to the thermodynamic temperature at which the liquid boils.