Table of Molar Enthalpies of Fusion and Vaporization
/ kJ mol1
|Melting Point / K||ΔH(vaporization) / kJ mol-1||Boiling Point / K||(ΔHv/Tb)|
/ JK-1 mol-1
|Water*||H2O||6.00678 at 0°C, 101kPa|
6.354 at 81.6 °C, 2.50 MPa
|273.1||40.657 at 100 °C, |
45.051 at 0 °C,
46.567 at -33 °C
This is a table of Molar Enthalpies of Fusion and Vaporization for a set of common substances. When heated, a solidA state of matter having a specific shape and volume and in which the particles do not readily change their relative positions. will increase in temperatureA physical property that indicates whether one object can transfer thermal energy to another object. until it reaches its meltingThe process of a liquid forming from a solid. point. Then, temperature will cease to rise, and heat energyA system's capacity to do work. will be supplied to the process of separating the molecules and forming a liquidA state of matter in which the atomic-scale particles remain close together but are able to change their positions so that the matter takes the shape of its container phase.
In the same way, when a liquid reaches its boilingThe process of a liquid becoming vapor in which bubbles of vapor form beneath the surface of the liquid; at the boiling temperature the vapor pressure of the liquid equals the pressure of the gas in contact with the liquid. point, the temperature will cease to rise, and energy will be supplied to the process of separating molecules into the gasA state of matter in which a substance occupies the full volume of its container and changes shape to match the shape of the container. In a gas the distance between particles is much greater than the diameters of the particles themselves; hence the distances between particles can change as necessary so that the matter uniformly occupies its container. phase. This table shows the amount of energy needed to do this for a mole of each substance.
This table is found on Enthalpy of Fusion and Enthalpy of Vaporization.