Table of Molar Enthalpies of Fusion and Vaporization

From ChemPRIME

Substance	Formula	ΔH(fusion) / kJ mol1	Melting Point / K	ΔH(vaporization) / kJ mol-1	Boiling Point / K	(ΔHv/Tb) / JK-1 mol-1
Neon	Ne	0.33	24	1.80	27	67
Oxygen	O2	0.44	54	6.82	90.2	76
Methane	CH4	0.94	90.7	8.18	112	73
Ethane	C2H6	2.85	90.0	14.72	184	80
Chlorine	Cl2	6.40	172.2	20.41	239	85
Carbon tetrachloride	CCl4	2.67	250.0	30.00	350	86
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	373.1	109
n-Nonane	C9H20	19.3	353	40.5	491	82
Mercury	Hg	2.30	234	58.6	630	91
Sodium	Na	2.60	371	98	1158	85
Aluminum	Al	10.9	933	284	2600	109
Lead	Pb	4.77	601	178	2022	88

*http://www1.lsbu.ac.uk/water/data.html

This is a table of Molar Enthalpies of Fusion and Vaporization for a set of common substances. When heated, a solid will increase in temperature until it reaches its melting point. Then, temperature will cease to rise, and heat energy will be supplied to the process of separating the molecules and forming a liquid phase.

In the same way, when a liquid reaches its boiling point, the temperature will cease to rise, and energy will be supplied to the process of separating molecules into the gas 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.