Download Table 1. Thermodynamic data at 25oC for assorted inorganic ... and more Lecture notes Chemical Thermodynamics in PDF only on Docsity!
Tables:
Table 1. Thermodynamic data at 25 o^ C for assorted inorganic substances.
Substance
Enthalpy of formation ∆ H (^) f^0 , kJ/mol
Free energy of formation ∆ G (^) f^0 , kJ/mol
Entropy S^0 , J/(K·mol)
Aluminum Al( s ) 0 0 28. Al3+( aq ) -524.7 -481.2 -321. Al 2 O 3 ( s ) -1675.7 -1582.3 50. Al(OH) 3 ( s ) -1276 --- --- AlCl 3 ( s ) -704.2 -628.8 110. Antimony SbH 3 ( g ) 145.11 147.75 232. SbCl 3 ( g ) -313.8 -301.2 337. SbCl 5 ( g ) -394.34 -334.29 401. Arsenic As( s, gray ) 0 0 35. As 2 S 3 ( s ) -169.0 -168.6 163. AsO 4 3-^ ( aq ) -888.14 -648.41 -162. Barium Ba( s ) 0 0 62. Ba 2+( aq ) -537.64 -560.77 9. BaO( s ) -553.5 -525.1 70. BaCO 3 ( s ) -1216.3 -1137.6 112. BaCO 3 ( aq ) -1214.78 -1088.59 -47. Boron B( s ) 0 0 5. B 2 O 3 ( s ) -1272.8 -1193.7 53. BF 3 ( g ) -1137.0 -1120.3 254. Bromine Br 2 ( l ) 0 0 152. Br 2 ( g ) 30.91 3.11 245. Br( g ) 111.88 82.40 175. Br – ( aq ) -121.55 -103.96 82. HBr( g ) -36.40 -53.45 198. Calcium Ca( s ) 0 0 41. Ca( g ) 178.2 144.3 154. Ca 2+( aq ) -542.83 -553.58 -53. CaO( s ) -635.09 -604.03 39. Ca(OH) 2 ( s ) -986.09 -898.49 83. Ca(OH) 2 ( aq ) -1002.82 -868.07 -74.
Table 1. Thermodynamic data at 25 o^ C for assorted inorganic substances (continued).
Substance
Enthalpy of formation ∆ H (^) f^0 , kJ/mol
Free energy of formation ∆ G (^) f^0 , kJ/mol
Entropy S^0 , J/(K·mol)
CaCO 3 ( s, calcite ) -1206.9 -1128.8 92. CaCO 3 ( s,aragonite ) -1207.1 -1127.8 88. CaCO 3 ( aq ) -1219.97 -1081.39 -110. CaF 2 ( s ) -1219.6 -1167.3 68. CaF 2 ( aq ) -1208.09 -1111.15 -80. CaCl 2 ( s ) -795.8 -748.1 104. CaCl 2 ( aq ) -877.1 -816.0 59. CaBr 2 ( s ) -682.8 -663.6 130 CaC 2 ( s ) -59.8 -64.9 69. CaSO 4 ( s ) -1434.11 -1321.79 106. CaSO 4 ( aq ) -1452.10 -1298.10 -33. Carbon C( s, graphite ) 0 0 5. C( s, diamond ) 1.895 2.900 2. C( g ) 716.68 671.26 158. CO( g ) -110.53 -137.17 197. CO 2 ( g ) -393.51 -394.36 213. CO 3 2-^ ( aq ) -677.14 -527.81 -56. CCl 4 ( l ) -135.44 -65.21 216. CS 2 ( l ) 89.70 65.27 153. HCN( g ) 135.1 124.7 201. HCN( l ) 108.87 124.97 112. Cerium Ce( s ) 0 0 72. Ce 3+( aq ) -696.2 -672.0 - Ce 4+( aq ) -537.2 -503.8 - Chlorine Cl 2 ( g ) 0 0 223. Cl( g ) 121.68 105.68 165. Cl–( aq ) -167.16 -131.23 56. HCl( g ) -92.31 -95.30 186. HCl( aq ) -167.16 -131.23 56. Copper Cu( s ) 0 0 33. Cu +( aq ) 71.67 49.98 40. Cu 2+( aq ) 64.77 65.49 -99. Cu 2 O( s ) -168.6 -146.0 93. CuO( s ) -157.3 -129.7 42. CuSO 4 ( s ) -771.36 -661.8 109
Table 1. Thermodynamic data at 25 o^ C for assorted inorganic substances (continued).
Substance
Enthalpy of formation ∆ H (^) f^0 , kJ/mol
Free energy of formation ∆ G (^) f^0 , kJ/mol
Entropy S^0 , J/(K·mol)
Mg( g ) 147.70 113.10 148. Mg 2+( aq ) -466.85 -454.8 -138. MgO( s ) -601.70 -569.43 26. MgCO 3 ( s ) -1095.8 -1012.1 65. MgBr 2 ( s ) -524.3 -503.8 117. Mercury Hg( l ) 0 0 76. Hg( g ) 61.32 31.82 174. HgO( s ) -90.83 -58.54 70. Hg 2 Cl 2 ( s ) -265.22 -210.75 192. Nitrogen N 2 ( g ) 0 0 191. NO( g ) 90.25 86.55 210. N 2 O( g ) 82.05 104.20 219. NO 2 ( g ) 33.18 51.31 240. N 2 O 4 ( g ) 9.16 97.89 304. HNO 3 ( l ) -174.10 -80.71 155. HNO 3 ( aq ) -207.36 -111.22 146. NO 3 – ( aq ) -205.0 -108.74 146. NH 3 ( g ) -46.11 -16.45 192. NH 3 ( aq ) -80.29 -26.50 111. NH 4 +( aq ) -132.51 -79.31 113. NH 2 OH( s ) -114.2 --- --- HN 3 ( g ) 294.1 328.1 238. N 2 H 4 ( l ) 50.63 149.34 121. NH 4 NO 3 ( s ) -365.56 -183.87 151. NH 4 Cl( s ) -314.43 -202.87 94. NH 4 ClO 4 ( s ) -295.31 -88.75 186. Oxygen O 2 ( g ) 0 0 205. O 3 ( g ) 142.7 163.2 238. OH – ( aq ) -229.99 -157.24 -10. Phosphorus P( s, white ) 0 0 41. P 4 ( g ) 58.91 24.44 279. PH 3 ( g ) 5.4 13.4 210. P 4 O 10 ( s ) -2984.0 -2697.0 228. H 3 PO 3 ( aq ) -964.0 --- --- H 3 PO 4 ( l ) -1266.9 --- ---
Table 1. Thermodynamic data at 25 o^ C for assorted inorganic substances (continued).
Substance
Enthalpy of formation ∆ H (^) f^0 , kJ/mol
Free energy of formation ∆ G (^) f^0 , kJ/mol
Entropy S^0 , J/(K·mol)
H 3 PO 4 ( aq ) -277.4 -1018.7 --- PCl 3 ( l ) -319.7 -272.3 217. PCl 3 ( g ) -287.0 -267.8 311. PCl 5 ( g ) -374.9 -305.0 364. PCl 5 ( s ) -443.5 --- --- Potassium K( s ) 0 0 64. K( g ) 89.24 60.59 160. K+( aq ) -252.38 -283.27 102. KOH( s ) -424.76 -379.08 78. KOH( aq ) -482.37 -440.50 91. KF( s ) -567.27 -537.75 66. KCl( s ) -436.75 -409.14 82. KBr( s ) -393.80 -380.66 95. KI( s ) -327.90 -324.89 106. KClO 3 ( s ) -397.73 -296.25 143. KClO 4 ( s ) -432.75 -303.09 151. K 2 S( s ) -380.7 -364.0 105 K 2 S( aq ) -471.5 -480.7 190. Silicon Si( s ) 0 0 18. SiO 2 ( s, α) -910.94 -856.64 41. Silver Ag( s ) 0 0 42. Ag +( aq ) 105.58 77.11 72. Ag 2 O( s ) -31.05 -11.20 121. AgBr( s ) -100.37 -96.90 107. AgBr( aq ) -15.98 -26.86 155. AgCl( s ) -127.7 -109.79 96. AgCl( aq ) -61.58 -54.12 129. AgI( s ) -61.84 -66.19 115. AgI( aq ) 50.38 25.52 184. AgNO 3 ( s ) -124.39 -33.41 140. Sodium Na( s ) 0 0 51. Na( g ) 107.32 76.76 153. Na +( aq ) -240.12 -261.91 59. NaOH( s ) -425.61 -379.49 64. NaOH( aq ) -470.11 -419.15 48.
Table 2.
Thermodynamic data at 25
o^ C for assorted organic substances.
Substance
Enthalpy of combustion
∆^
(^0) H c , kJ/mol
Enthalpy of formation
∆^ H
0 , kJ/molf
Free energy of formation
∆^
G^
0 , kJ/molf
Entropy (^0) S , J/(K·mol)
Hydrocarbons CH
( g 4
),^
methane
C^2
H^2
( g
),^
acethylene
C^2
H^4
( g
),^
ethylene
C^2
H^6
( g
),^
ethane
C^3
H^6
( g
),^
propylene
C^3
H^6
( g
),^
cyclopropane
C^3
H^8
( g
),^
propane
C^4
H^10
( g
),^
butane
C^5
H^12
( g
),^
pentane
C^6
H^6
( l ),
benzene
C^6
H^6
( g
)^
C^7
H^8
( l ),
toluene
C^7
H^8
( g
)^
C^6
H^12
( l ),
cyclohexane
C^6
H^12
( g
)^
C^8
H^18
( l ),
octane
Alcohols, phenols CH
OH( 3
l ),
methanol
CH
OH( 3
g )
C^2
H^5
OH(
l ), ethanol
C^2
H^5
OH(
g )
C^6
H^5
OH(
s ),
phenol
Table 2.
Thermodynamic data at 25
o^ C for assorted organic substances (continued).
Substance
Enthalpy of combustion
∆^
(^0) H c , kJ/mol
Enthalpy of formation
∆^ H
0 , kJ/molf
Free energy of formation
∆^
G^
0 , kJ/molf
Entropy (^0) S , J/(K·mol)
Aldehydes, ketones HCHO (
g ),
formaldehyde
CH
CHO ( 3
l ),
acetaldehyde
CH
CHO ( 3
g )
CH
COCH 3
l ),
acetone
Carboxylic acids HCOOH (
l ),
formic acid
CH
COOH ( 3
l ),
acetic acid
CH
COOH ( 3
aq
)^
(COOH)
s ),
oxalic acid
C^6
H^5
COOH (
s ),
benzoic acid
Sugars C^6
H^12
O
s ),
glucose
C^6
H^12
O
aq
)^
C^6
H^12
O
s ),
fructose
C^12
H
O 22
11
( s
),^
sucrose
Nitrogen compounds CO(NH
)^22
( s
),^
urea
C^6
H^5
NH
l ), aniline
NH
CH 2
COOH( 2
s ),
glycine
CH
NH 3
g ),
methylamine
Table 3. Standard reduction potentials at 25 o^ C (electrochemical series; continued).
strongest reducer
Table 4. Standard reduction potentials at 25 o^ C (in alphabetical order by redox couple).
Table 4. Standard reduction potentials at 25 o^ C (in alphabetical order by redox couple; continued).
