Appendix H
See Table H.1.
Table H.1 Standard Enthalpy and Entropy of formation of some products. The standard Gibbs
Free Energy of formation DG° can be calculated by using the DG° = DH° − TDS° equation, where
T is the temperature in K
Substance
State
DH° f
kJ
mol
S°
J
mol K
Substance
State
DH° f
kJ
mol
S°
J
mol K
Ag
s
0
42.6
Cl 2
g
0
223.0
Ag+
aq
105.79
72.7
Cl
−
aq
−167.080
56.5
AgCl
s
−127.01
96.2
ClO 4
−
aq
−128.10
182.0
AgBr
s
−100.4
107.1
Cr
s
0
23.8
AgNO 3
s
−124.4
140.9
Cr 2 O 3
g
−1139.7
81.2
A1
s
0
28.3
Cu
s
0
33.2
A1
+3
aq
−538.4
−321.7
Cu
+
aq
+71.7
40.6
AlCl 3
s
−704
110.7
Cu
+2
aq
+64.8
−99.6
A1 2 O 3
s
−1675.7
50.9
CuO
s
−157.3
42.6
Ba
s
0
62.8
Cu 2 O
s
−168.6
93.1
BaCl 2
s
−858.6
123.7
CuS
s
−53.1
66.5
BaCO 3
s
−1216.3
112.1
Cu 2 S
s
−79.5
120.9
Ba(NO 3 ) 2
s
−992
214
CuSO 4
s
−771.4
107.6
BaO
s
−553.5
70.4
F
−
aq
−335.35
−13.8
Ba(OH) 2
s
−998.2
112
F 2
g
0
202.7
BaSO 4
s
−1473.2
132.2
Fe
s
0
27.3
Br 2
l
0
152.2
Fe(OH) 3
s
−823.0
106.7
C
s
0
5.7
Fe 2 O 3
s
−824.2
87.4
CCl 4
l
−135.4
216.4
Fe 3 O 4
s
−1118.4
146.4
CHCl 3
l
−134.5
201.7
H 2
g
0
130.6
CH 4
g
−74.8
186.2
H
+
aq
0
0.0
a
C 2 H 2
g
+226.7
200.8
HBr
g
−36.29
198.6
(continued)
© Springer Nature Switzerland AG 2021
M. Aresta and A. Dibenedetto, The Carbon Dioxide Revolution,
https://doi.org/10.1007/978-3-030-59061-1
247