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Heats of Formation

Thermochemistry Heats of Formation Table for Common Compounds

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The molar heat of formation of a compound (ΔHf) is equal to its enthalpy change (ΔH) when one mole of compound is formed at 25°C and 1 atm from elements in their stable form. This is a table of the heats of formation for a variety of common compounds. As you can see, most heats of formation are negative quantities, which implies that the formation of a compound from its elements usually is an exothermic process.

Reference: Masterton, Slowinski, Stanitski, Chemical Principles, CBS College Publishing, 1983.

Table of Heats of Formation

Compound ΔHf (kJ/mol) Compound ΔHf (kJ/mol)
AgBr(s) -99.5 C2H2(g) +226.7
AgCl(s) -127.0 C2H4(g) +52.3
AgI(s) -62.4 C2H6(g) -84.7
Ag2O(s) -30.6 C3H8(g) -103.8
Ag2S(s) -31.8 n-C4H10(g) -124.7
Al2O3(s) -1669.8 n-C5H12(l) -173.1
BaCl2(s) -860.1 C2H5OH(l) -277.6
BaCO3(s) -1218.8 CoO(s) -239.3
BaO(s) -558.1 Cr2O3(s) -1128.4
BaSO4(s) -1465.2 CuO(s) -155.2
CaCl2(s) -795.0 Cu2O(s) -166.7
CaCO3 -1207.0 CuS(s) -48.5
CaO(s) -635.5 CuSO4(s) -769.9
Ca(OH)2(s) -986.6 Fe2O3(s) -822.2
CaSO4(s) -1432.7 Fe3O4(s) -1120.9
CCl4(l) -139.5 HBr(g) -36.2
CH4(g) -74.8 HCl(g) -92.3
CHCl3(l) -131.8 HF(g) -268.6
CH3OH(l) -238.6 HI(g) +25.9
CO(g) -110.5 HNO3(l) -173.2
CO2(g) -393.5 H2O(g) -241.8
H2O(l) -285.8 NH4Cl(s) -315.4
H2O2(l) -187.6 NH4NO3(s) -365.1
H2S(g) -20.1 NO(g) +90.4
H2SO4(l) -811.3 NO2(g) +33.9
HgO(s) -90.7 NiO(s) -244.3
HgS(s) -58.2 PbBr2(s) -277.0
KBr(s) -392.2 PbCl2(s) -359.2
KCl(s) -435.9 PbO(s) -217.9
KClO3(s) -391.4 PbO2(s) -276.6
KF(s) -562.6 Pb3O4(s) -734.7
MgCl2(s) -641.8 PCl3(g) -306.4
MgCO3(s) -1113 PCl5(g) -398.9
MgO(s) -601.8 SiO2(s) -859.4
Mg(OH)2(s) -924.7 SnCl2(s) -349.8
MgSO4(s) -1278.2 SnCl4(l) -545.2
MnO(s) -384.9 SnO(s) -286.2
MnO2(s) -519.7 SnO2(s) -580.7
NaCl(s) -411.0 SO2(g) -296.1
NaF(s) -569.0 So3(g) -395.2
NaOH(s) -426.7 ZnO(s) -348.0
NH3(g) -46.2 ZnS(s) -202.9

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