This document provides a table of standard enthalpies of formation (ΔHformation) in kJ/mol for various common substances. It notes that Hess's law can be used to calculate the standard enthalpy of a reaction (ΔHrx) from the standard enthalpies of formation of the products and reactants. The table lists the ΔHformation values for over 30 different elements and compounds.

1. C06 Enthalpy Table
Standard Heats of Formation, ΔHformation
Hess’s Law, ΔHrx = ΣΔHformation products - ΣΔHformation reactants
Standard Enthalpy of
Formation Table
ΔHformation
Substance kJ/mol
Al(s) 0
Al2O3(s) -1670
C(s, graphite) 0
CO (g) -111
CO2 (g) -394
CH4 (g) -75
CH3OH (l) -239
C2H2 (g) 227
C2H4 (g) 52
C2H6 (g) -85
C2H5OH (l) -278
CaO (s) -636
Ca(OH)2 (s) -987
CaSO4(s) -1433
Cl2 (g) 0
Fe2O3 (s) -822
H2 (g) 0
HCl(g) -92
H2O (g) -242
H2O (l) -286
H2O2 (l) -188
H2SO4 (l) -811
Hg (l) 0
Hg (g) 61
MgO(s) -602
N2 (g) 0
NH3 (g) -46
NH4Cl(s) -315
N2O (g) 82
N2O4 (g) 10
NaCl (s) -411
NaOH (s) -427
O2 (g) 0
P4O10(s) -2980
S(s) 0
SO2 (g) -297
SO3 (g) -395