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Appendix — Reference Tables Table A1

Atomic Masses of the Elements

Table A2

Names, Formulas, and Charges of Some Common Ions

Table A3

Solubility of Common Compounds in Water

Table A4

Solubility Product Constants at 25°C

Table A5

Relative Strengths of Brønsted-Lowry Acids and Bases

Table A6

Acid-Base Indicators

Table A7

Standard Reduction Potentials of Half-Cells

Table A8

Thermodynamic Data at 25°C for Assorted Substances

— Reference Tables 516 Appendix

ATOMIC MASSES OF THE ELEMENTS

Table A1 Atomic Masses12 of the Elements

Based on mass of C at 12.00. Based on of carbon-12 at 12.00. Values in parentheses aremass the mass number of the most stable or best For elements that do not occur naturally, the atomic of thethat most or best known isotope is shown in parentheses. known isotopes formass elements dostable not occur naturally. Element Actinium Aluminum Americium Antimony Argon Arsenic Astatine Barium Berkelium Beryllium Bismuth Boron Bromine Cadmium Calcium Californium Carbon Cerium Cesium Chlorine Chromium Cobalt Copper Curium Dubnium Dysprosium Einsteinium Erbium Europium Fermium Fluorine Francium Gadolinium Gallium Germanium Gold Hafnium Helium Holmium Hydrogen Indium Iodine Iridium Iron Krypton Lanthanum Lawrencium Lead Lithium Lutetium Magnesium Manganese Mendelevium

Symbol

Atomic Number

Atomic Mass

Ac Al Am Sb Ar As At Ba Bk Be Bi B Br Cd Ca Cf C Ce Cs Cl Cr Co Cu Cm Db Dy Es Er Eu Fm F Fr Gd Ga Ge Au Hf He Ho H In I Ir Fe Kr La Lr Pb Li Lu Mg Mn Md

89 13 95 51 18 33 85 56 97 4 83 5 35 48 20 98 6 58 55 17 24 27 29 96 105 66 99 68 63 100 9 87 64 31 32 79 72 2 67 1 49 53 77 26 36 57 103 82 3 71 12 25 101

(227) 27.0 (243) 121.8 39.9 74.9 (210) 137.3 (247) 9.0 209.0 10.8 79.9 112.4 40.1 (251) 12.0 140.1 132.9 35.5 52.0 58.9 63.5 (247) (262) 162.5 (252) 167.3 152.0 (257) 19.0 (223) 157.3 69.7 72.6 197.0 178.5 4.0 164.9 1.0 114.8 126.9 192.2 55.8 83.8 138.9 (262) 207.2 6.9 175.0 24.3 54.9 (258)

Element Mercury Molybdenum Neodymium Neon Neptunium Nickel Niobium Nitrogen Nobelium Osmium Oxygen Palladium Phosphorus Platinum Plutonium Polonium Potassium Praseodymium Promethium Protactinium Radium Radon Rhenium Rhodium Rubidium Ruthenium Rutherfordium Samarium Scandium Selenium Silicon Silver Sodium Strontium Sulfur Tantalum Technetium Tellurium Terbium Thallium Thorium Thulium Tin Titanium Tungsten Uranium Vanadium Xenon Ytterbium Yttrium Zinc Zirconium

Symbol

Atomic Number

Atomic Mass

Hg Mo Nd Ne Np Ni Nb N No Os O Pd P Pt Pu Po K Pr Pm Pa Ra Rn Re Rh Rb Ru Rf Sm Sc Se Si Ag Na Sr S Ta Tc Te Tb Tl Th Tm Sn Ti W U V Xe Yb Y Zn Zr

80 42 60 10 93 28 41 7 102 76 8 46 15 78 94 84 19 59 61 91 88 86 75 45 37 44 104 62 21 34 14 47 11 38 16 73 43 52 65 81 90 69 50 22 74 92 23 54 70 39 30 40

200.6 95.9 144.2 20.2 (237) 58.7 92.9 14.0 (259) 190.2 16.0 106.4 31.0 195.1 (244) (209) 39.1 140.9 (145) 231.0 (226) (222) 186.2 102.9 85.5 101.1 (261) 150.4 45.0 79.0 28.1 107.9 23.0 87.6 32.1 180.9 (98) 127.6 158.9 204.4 232.0 168.9 118.7 47.9 183.8 238.0 50.9 131.3 173.0 88.9 65.4 91.2

Table A2 Names, Formulas, and Charges Some NAMES, FORMULAE, AND C HARGES OF of SOME CCommon OMMON IIons ONS * Aqueous solutions readily oxidized by air * Aqueous solutions are readily oxidized by air. ** Notinstable in aqueous solutions ** Not stable aqueous solutions. Positive Ions (Cations) Al3+

Aluminum

Pb4+

NH4+

Ammonium

Li+

Barium

Magnesium

Manganese(II), manganous

Calcium

Cr2+

Chromium(II), chromous

Mn4+

Cu2+ H

H3O

Fe2+ 3+

Fe Pb

Mercury(I)*, mercurous

Mercury(II), mercuric

Copper(I)*, cuprous

K+

Copper(II), cupric

Potassium

Silver

Hydrogen

Manganese(IV)

Hg2

Chromium(III), chromic

Lithium

Lead(IV), plumbic

Hydronium

Sodium

Iron(II)*, ferrous

Sn2+

Tin(II)*, stannous

Tin(IV), stannic

Zinc

Bromide

OH–

Hydroxide

Carbonate

ClO–

Hypochlorite

Iron(III), ferric Lead(II), plumbous Negative Ions (Anions)

Br– CO32– –

ClO3

–

ClO2– 2–

CrO4

–

Cr2O72– –

H2PO4 CH3COO

–

F– –

HCO3

–

HC2O4

HSO4–

Chlorate

Chloride

2–

Chlorite Chromate Cyanide Dichromate Dihydrogen phosphate Ethanoate, acetate Fluoride Hydrogen carbonate, bicarbonate Hydrogen oxalate, binoxalate

HPO4

Nitrate Nitrite

NO2

2–

C2O4

O2–

Oxide** Perchlorate

–

Permanganate

ClO4 MnO4

PO4?–

Phosphate

2–

Sulfate

2–

Sulfide

SO4 S

Oxalate

–

Hydrogen sulfide, bisulfide

–

Hydrogen sulfite, bisulfite

— Reference Tables 518 Appendix

Monohydrogen phosphate

–

SO32–

HSO3

Iodide

NO3–

Hydrogen sulfate, bisulfate

Chemistry 12

–

SCN

Sulfite Thiocyanate

Data Page

SOLUBILITY OF COMMON COMPOUNDS IN WATER Table A3 Solubility of Common Compounds in Water The term soluble means > 0.1atmol /L at 25°C. “Soluble”here means > 0.1 mol/L 25°C.

Solubility of Compounds

All

Alkali ions: Li+, Na+, K+, Rb+, Cs+, Fr+

Soluble

All

Hydrogen ion: H+

Soluble

All

Ammonium ion: NH4+

Soluble

Nitrate, NO3–

All

Soluble

All others

Soluble

Chloride, Cl– Bromide, Br– Iodide, I–

123

Positive Ions (Cations)

14243

Negative Ions (Anions)

2–

123

Sulfate, SO4

2–

123

Sulfide, S

–

Hydroxide, OH

14253

Phosphate, PO43–

2–

Carbonate, CO3 Sulfite, SO32–

Ag+, Pb2+, Cu+ All others

Low Solubility Soluble

Ag+, Ca2+, Sr2+, Ba2+, Pb2+ Alkali ions, H+, NH4+, Be2+, Mg2+, Ca2+, Sr2+, Ba2+

Low Solubility Soluble

All others

Alkali ions, H+, NH4+, Sr2+

Low Solubility Soluble Low Solubility

All others

Alkali ions, H+, NH4+ All others

Soluble Low Solubility

SOLUBILITY PRODUCT CONSTANTS AT 25°C Table A4 Solubility Product Constants at 25°C

Name

Formula

K sp

Barium carbonate

BaCO3

2.6 10–9

Barium chromate

BaCrO4

1.2 10–10

Barium sulfate

BaSO4

1.1 10–10

Calcium carbonate

CaCO3

5.0 10–9

Calcium oxalate

CaC2O4

2.3 10–9

Calcium sulfate

CaSO4

7.1 10–5

Copper(I) iodide

CuI

1.3 10–12

Copper(II) iodate

Cu(IO3)2

6.9 10–8

Copper(II) sulfide

CuS

6.0 10–37

Iron(II) hydroxide

Fe(OH)2

4.9 10–17

Iron(II) sulfide

FeS

6.0 10–19

Iron(III) hydroxide

Fe(OH)3

2.6 10–39

Lead(II) bromide

PbBr2

6.6 10–6

Lead(II) chloride

PbCl2

1.2 10–5

Lead(II) iodate

Pb(IO3)2

3.7 10–13

Lead(II) iodide

PbI2

8.5 10–9

Lead(II) sulfate

PbSO4

1.8 10–8

Magnesium carbonate

MgCO3

6.8 10–6

Magnesium hydroxide

Mg(OH)2

5.6 10–12

Silver bromate

AgBrO3

5.3 10–5

Silver bromide

AgBr

5.4 10–13

Silver carbonate

Ag2CO3

8.5 10–12

Silver chloride

AgCl

1.8 10–10

Silver chromate

Ag2CrO4

1.1 10–12

Silver iodate

AgIO3

3.2 10–8

Silver iodide

AgI

8.5 10–17

Strontium carbonate

SrCO3

5.6 10–10

Strontium fluoride

SrF2

4.3 10–9

Strontium sulfate

SrSO4

3.4 10–7

Zinc sulfide

ZnS

2.0 10–25

— Reference Tables 520 Appendix 12 Chemistry

RELATIVE STRENGTHS OF BRØNSTED-LOWRY ACIDS AND BASES Table A5 RelativeinStrengths of Brønsted-Lowry aqueous solution at room temperature. Acids and Bases In aqueous solution at room temperature

STRONG

Name of Acid

Iodic Oxalic

H2C2O4 H 2 SO 3

Hydrogen sulfate ion

HSO 4 −

Phosphoric

H 3 PO 4

Citric Nitrous Hydrofluoric Methanoic, formic

Fe(H 2 O)6 3 + H 3C 6 H 5O 7 HNO 2 HF HCOOH

Hexaaquochromium ion, chromium(III) ion

Cr(H 2 O)6 3 +

Benzoic

C 6 H 5COOH

Hydrogen oxalate ion Ethanoic, acetic

HC 2 O 4 − CH 3COOH

Dihydrogen citrate ion

H 2 C 6 H 5O 7 −

Hexaaquoaluminum ion, aluminum ion

Al(H 2 O)6 3 +

Carbonic (CO 2 +H 2 O) Monohydrogen citrate ion Hydrogen sulfite ion Hydrogen sulfide Dihydrogen phosphate ion Boric Ammonium ion Hydrocyanic Phenol Hydrogen carbonate ion Hydrogen peroxide

H 2 CO 3 HC 6 H 5O 7

2−

HSO 3 − H 2S H 2 PO 4 − H 3 BO 3 NH 4 + HCN C 6 H 5OH HCO 3 − H2O2

→ → → → → → → ←

H+ H+ H+ H+ H+ H+ H+

+ ClO 4 − + I− + Br − + Cl − + NO 3 − + HSO 4 − + H2O

− + → ← H + IO 3 − + → ← H + HC 2 O 4 → H + + HSO − ← 3 2− + → + H SO ← 4 − + → H H PO + ← 2

1.2 × 10 − 2 7.5 × 10 − 3

+ − → ← H +F + − → ← H + HCOO + 2+ → ← H + Cr(H 2 O)5 (OH) + − → ← H + C H COO

3.5 × 10 − 4

2− + → ← H + C2O4 + − → ← H + CH 3COO 2− + → ← H + HC H O

6.4 × 10 − 5

+ 2+ → ← H + Al(H 2 O)5 (OH) − + → ← H + HCO 3 3− + → ← H +C H O

1.4 × 10 − 5

→ H + + SO ← 3 + − → + H HS ← + → ← H + HPO

1.0 × 10 − 7

5 7 2−

2−

→ H+ + C H O− ← 6 5 2− + → H CO + ← 3 − + → ← H + HO

← H + + O2 −

NH 3

← H + NH 2

4.6 × 10 − 4 1.8 × 10 − 4 1.5 × 10 − 4 6.5 × 10 − 5 1.8 × 10 − 5 1.7 × 10 − 5 4.3 × 10 − 7 4.1 × 10 − 7

6.2 × 10 − 8 7.3 × 10 −10 5.6 × 10 −10 4.9 × 10 −10 1.3 × 10 −10 5.6 × 10 −11 2.4 × 10 −12 2.2 × 10 −13 1.0 × 10 −14 very small

−

very small

STRONG

2 PO 4 3 − −

OH −

7.1 × 10 − 4

9.1 × 10 − 8

− + → ← H + H 2 BO 3 + → ← H + NH 3 + − → ← H + CN

Hydroxide ion

Data Page

1.5 × 10 − 2

6.0 × 10 − 3

H 2O

Ammonia

5.9 × 10 − 2

+ 2+ → ← H + Fe(H 2 O)5 (OH) − + → ← H + H 2 C 6 H 5O 7 − + → ← H + NO

Water

HPO 4 2 −

large large large large large large

1.7 × 10 −1

+ → ← H + + → ← H + OH

Monohydrogen phosphate ion

very very very very very very 1.0

STRENGTH OF BASE

STRENGTH OF ACID

HIO 3

Sulfurous (SO2 +H2O)

Hexaaquoiron ion, iron(III) ion

WEAK

HClO 4 HI HBr HCl HNO 3 H 2 SO 4 H 3O +

Base

WEAK

Perchloric Hydriodic Hydrobromic Hydrochloric Nitric Sulfuric Hydronium Ion

Acid

Chemistry 12

ACID-BASE INDICATORS Table A6 Acid-Base Indicators Indicator

Colour Change as pH Increases

Methyl violet

0.0 – 1.6

yellow to blue

Thymol blue

1.2 – 2.8

red to yellow

Orange IV

1.4 – 2.8

red to yellow

Methyl orange

3.2 – 4.4

red to yellow

Bromcresol green

3.8 – 5.4

yellow to blue

Methyl red

4.8 – 6.0

red to yellow

Chlorophenol red

5.2 – 6.8

yellow to red

Bromthymol blue

6.0 – 7.6

yellow to blue

Phenol red

6.6 – 8.0

yellow to red

Neutral red

6.8 – 8.0

red to amber

Thymol blue

8.0 – 9.6

yellow to blue

Phenolphthalein

8.2 – 10.0

colourless to pink

Thymolphthalein

9.4 – 10.6

colourless to blue

Alizarin yellow

10.1 – 12.0

yellow to red

Indigo carmine

11.4 – 13.0

blue to yellow

— Reference Tables 522 Appendix Chemistry 12

pH Range in Which Colour Change Occurs

Table A7 Standard Reduction Potentials OFof ALF-CELLS STANDARD REDUCTION POTENTIALS HHalf-Cells Ionicconcentrations concentrationsare areatat11M wateratat25°C. 25°C. Ionic M ininwater Oxidizing Agents F2 (g) + 2 e

−

STRONG

H 2 O 2 + 2H + + 2e − MnO 4 − + 8H + + 5e − Au 3+ + 3e − BrO 3 − + 6H + + 5e − ClO 4 − + 8H + + 8e − Cl 2 (g) + 2 e − Cr2 O 7 2 − + 14H + + 6e − 1 2

O 2 (g) + 2 H + + 2 e −

MnO 2 (s) + 4H + + 2 e − IO 3 − + 6H + + 5e − Br2 (l) + 2 e − −

AuCl 4 + 3e

−

NO 3 − + 4H + + 3e − Hg 2 + + 2 e − 1 2

O 2 (g) + 2 H (10 +

−7

M) + 2e −

2 NO 3 − + 4H + + 2 e − Ag + + e − 1 2

Hg 2 2 + + e −

STRENGTH OF OXIDIZING AGENT

O 2 (g) + 2 H + + 2 e − MnO 4 − + 2 H 2 O + 3e − I 2 (s) + 2 e − Cu + + e − H 2 SO 3 + 4H + + 4e − Cu 2 + + 2 e − SO 4 2 − + 4H + + 2 e − Cu 2 + + e − Sn 4 + + 2 e − S(s) + 2 H + + 2 e − 2H + + 2e − Pb 2 + + 2 e − Sn 2 + + 2 e − Ni 2 + + 2 e − H 3 PO 4 + 2 H + + 2 e − Co 2 + + 2 e − Se(s) + 2 H + + 2 e − Cr 3+ + e − 2H 2 O + 2e −

Overpotential Effect

Fe 2 + + 2 e − Ag 2 S(s) + 2 e − Cr 3+ + 3e − Zn 2 + + 2 e − Te(s) + 2 H + + 2 e − 2H 2 O + 2e − Mn 2 + + 2 e − Al 3+ + 3e − Mg 2 + + 2 e − Na + + e −

+1.78

2+ → ← Mn + 4H 2 O → ← Au(s) 1 → Br (l) + 3H O ←

+1.51

− → ← Cl + 4H 2 O − → ← 2Cl 3+ → 2 Cr + 7H O ←

+1.39

→ ← H2O 2+ → ← Mn + 2 H 2 O 1 → I ← 2 2 (s) + 3H 2 O − → ← 2 Br − → ← Au(s) + 4Cl → ( ) NO g 2 H + ← 2O → ← Hg(l)

→ ← H2O → ← N 2 O 4 + 2H 2 O → ← Ag(s)

+1.50 +1.48 +1.36 +1.23 +1.23 +1.22 +1.20 +1.09 +1.00 + 0.85 + 0.82 + 0.80 + 0.80

→ ← Hg(l) 2+ → ← Fe → ← H O

+ 0.77

− → ← MnO 2 (s) + 4OH − → 2 I ← → ← Cu(s)

+ 0.54

+ 0.80 + 0.70

→ ← S(s) + 3H 2 O → ← Cu(s) → ← H SO + H O 2

+ 0.60 + 0.52 + 0.45 + 0.34 + 0.17

+ → ← Cu 2+ → Sn ← → ← H S(g)

+ 0.15

→ ← H 2 (g) → ← Pb(s) → ← Sn(s)

+ 0.00

→ ← Ni(s) → ← H 3 PO 3 + H 2 O → ← Co(s)

+ 0.15 + 0.14 − 0.13 − 0.14 − 0.26 − 0.28 − 0.28

→ ← H 2 Se 2+ → ← Cr − −7 → ← H + 2 OH (10 M )

− 0.40

→ ← Fe(s) 2− → ← 2 Ag(s) + S → ← Cr(s)

− 0.45

→ ← Zn(s) → ← H 2 Te − → ← H 2 (g) + 2 OH → ( ) Mn s ←

− 0.76

→ ← Al(s) → ← Mg(s) → ← Na(s)

− 0.41 − 0.41 − 0.69 − 0.74 − 0.79 − 0.83 −1.19 −1.66 − 2.37 − 2.71

− 3.03

Li + + e −

→ Li(s) ←

− 3.04

K+ + e− Rb + + e −

− 2.89 − 2.91 − 2.98

STRONG

− 2.93

Cs + + e −

→ ← K(s) → ← Rb(s) → ← Cs(s)

Ba 2 + + 2e −

Overpotential Effect

+ 0.96

− 2.87

Sr 2 + + 2e −

WEAK

+ 2.87 + 2.01

→ ← Ca(s) → ← Sr(s) → ← Ba(s)

Ca 2 + + 2 e −

Data Page

E° (Volts)

STRENGTH OF REDUCING AGENT

Fe 3+ + e −

→ ← 2F 2− → ← 2SO 4 → 2 H O ← −

WEAK

S2 O 8 2 − + 2 e −

Reducing Agents

Chemistry 12

Table A8 Thermodynamic Data at 25°C for Assorted Substances Table A8-Inorganic Thermodynamic data at 25oC for assorted inorganic substances. Substance

Enthalpy of formation 0 ∆ Hf

, kJ/mol

Free energy of formation 0 ∆ Gf ,

kJ/mol

Entropy 0

S , J/(K·mol)

Aluminum Al(s)

28.33

Al (aq)

-524.7

-481.2

-321.7

Al2O3(s)

-1675.7

-1582.3

50.92

Al(OH)3(s)

-1276

---

AlCl3(s)

-704.2

-628.8

110.67

SbH3(g)

145.11

147.75

232.78

SbCl3(g)

-313.8

-301.2

337.80

SbCl5(g)

-394.34

-334.29

401.94

35.1

-169.0

-168.6

163.6

-888.14

-648.41

-162.8

Antimony

Arsenic As(s, gray) As2S3(s) 3-

AsO4 (aq) Barium Ba(s)

62.8

Ba (aq)

-537.64

-560.77

9.6

BaO(s)

-553.5

-525.1

70.42

BaCO3(s)

-1216.3

-1137.6

112.1

BaCO3(aq)

-1214.78

-1088.59

-47.3

5.86

B2O3(s)

-1272.8

-1193.7

53.97

BF3(g)

-1137.0

-1120.3

254.12

Br2(l)

152.23

Br2(g)

30.91

3.11

245.46

Br(g)

111.88

82.40

175.02

–

Br (aq)

-121.55

-103.96

82.4

HBr(g)

-36.40

-53.45

198.70

Ca(s)

41.42

Ca(g)

Boron B(s)

Bromine

Calcium 178.2

144.3

154.88

Ca (aq)

-542.83

-553.58

-53.1

CaO(s)

-635.09

-604.03

39.79

Ca(OH)2(s)

-986.09

-898.49

83.39

Ca(OH)2(aq)

-1002.82

-868.07

-74.5

— Reference Tables 524 Appendix

Table A8-Inorganic Thermodynamic data at 25oC for assorted inorganic substances (continued). Substance

Enthalpy of formation 0 ∆ Hf

, kJ/mol

Free energy of formation 0 ∆ Gf ,

kJ/mol

Entropy S0, J/(K·mol)

CaCO3(s, calcite)

-1206.9

-1128.8

92.9

CaCO3(s,aragonite)

-1207.1

-1127.8

88.7

CaCO3(aq)

-1219.97

-1081.39

-110.0

CaF2(s)

-1219.6

-1167.3

68.87

CaF2(aq)

-1208.09

-1111.15

-80.8

CaCl2(s)

-795.8

-748.1

104.6

CaCl2(aq)

-877.1

-816.0

59.8

CaBr2(s)

-682.8

-663.6

130

CaC2(s)

-59.8

-64.9

69.96

CaSO4(s)

-1434.11

-1321.79

106.7

CaSO4(aq)

-1452.10

-1298.10

-33.1

C(s, graphite)

5.740

C(s, diamond)

1.895

2.900

2.377

C(g)

716.68

671.26

158.10

CO(g)

-110.53

-137.17

197.67

CO2(g)

-393.51

-394.36

213.74

CO3 (aq)

-677.14

-527.81

-56.9

CCl4(l)

-135.44

-65.21

216.40

CS2(l)

89.70

65.27

153.34

HCN(g)

135.1

124.7

201.78

HCN(l)

108.87

124.97

112.84

Carbon

Cerium Ce(s)

72.0

-696.2

-672.0

-205

-537.2

-503.8

-301

Cl2(g)

223.07

Cl(g)

121.68

105.68

165.20

–

Cl (aq)

-167.16

-131.23

56.5

HCl(g)

-92.31

-95.30

186.91

HCl(aq)

-167.16

-131.23

56.5

Ce (aq) Ce (aq) Chlorine

Copper Cu(s)

33.15

Cu (aq)

71.67

49.98

40.6

Cu (aq)

64.77

65.49

-99.6

Cu2O(s)

-168.6

-146.0

93.14

CuO(s)

-157.3

-129.7

42.63

CuSO4(s)

-771.36

-661.8

109

Table A8-Inorganic Thermodynamic data at 25oC for assorted inorganic substances (continued). Substance

Enthalpy of formation 0 ∆ Hf

, kJ/mol

Free energy of formation 0 ∆ Gf ,

kJ/mol

Entropy 0

S , J/(K·mol)

Fluorine F2(g)

202.78

F (aq)

-332.63

-278.79

-13.8

HF(g)

-271.1

-273.2

173.78

HF(aq)

-332.36

-278.79

-13.8

H2(g)

130.68

H(g)

217.97

203.25

114.71

H (aq)

H2O(l)

-285.83

-237.13

69.91

H2O(g)

-241.82

-228.57

188.83

H2O2(l)

-187.78

-120.35

109.6

H2O2(aq)

-191.17

-134.03

143.9

D2(g)

144.96

D2O(l)

-294.60

-243.44

75.94

D2O(g)

-249.20

-234.54

198.34

I2(s)

116.14

I2(g)

62.44

19.33

260.69

I (aq)

-55.19

-51.57

111.3

HI(g)

26.48

1.70

206.59

–

Hydrogen

Iodine

–

Iron Fe(s)

27.28

-89.1

-78.90

-137.7

-48.5

-4.7

-315.9

Fe3O4(s, magnetite)

-1118.4

-1015.4

146.4

Fe2O3(s, hematite)

-824.2

-742.2

87.40

FeS(s,α)

-100.0

-100.4

60.29

FeS(aq)

---

6.9

---

FeS2(s)

-178.2

-166.9

52.93

Fe (aq) Fe (aq)

Lead Pb(s)

64.81

Pb (aq)

-1.7

-24.43

10.5

PbO2(s)

-277.4

-217.33

68.6

PbSO4(s)

-919.94

-813.14

148.57

PbBr2(s)

-278.7

-261.92

161.5

PbBr2(aq)

-244.8

-232.34

175.3

32.68

Magnesium Mg(s) — Reference Tables 526 Appendix

Table A8-Inorganic Substance Mg(g)

Thermodynamic data at 25 Enthalpy of formation 0 ∆ Hf

, kJ/mol

C for assorted inorganic substances (continued). Free energy of formation 0 ∆Gf

, kJ/mol

Entropy 0

S , J/(K·mol)

147.70

113.10

148.65

Mg (aq)

-466.85

-454.8

-138.1

MgO( s )

-601.70

-569.43

26.94

MgCO 3(s )

-1095.8

-1012.1

65.7

MgBr 2(s )

-524.3

-503.8

117.2

Hg( l)

76.02

Hg( g)

61.32

31.82

174.96

HgO( s )

-90.83

-58.54

70.29

Hg 2Cl 2(s )

-265.22

-210.75

192.5

Mercury

Nitrogen N 2(g)

191.61

NO( g)

90.25

86.55

210.76

N 2O( g)

82.05

104.20

219.85

NO 2(g)

33.18

51.31

240.06

N 2O 4(g)

9.16

97.89

304.29

HNO 3(l)

-174.10

-80.71

155.60

HNO 3(aq)

-207.36

-111.22

146.4

–

NO 3 (aq)

-205.0

-108.74

146.4

NH 3(g)

-46.11

-16.45

192.45

NH 3(aq)

-80.29

-26.50

111.3

NH 4 (aq)

-132.51

-79.31

113.4

NH 2OH( s )

-114.2

---

HN 3(g)

294.1

328.1

238.97

N 2H 4(l)

50.63

149.34

121.21

NH 4NO 3(s )

-365.56

-183.87

151.08

NH 4Cl( s )

-314.43

-202.87

94.6

NH 4ClO 4(s )

-295.31

-88.75

186.2

O 2(g)

205.14

O 3(g)

142.7

163.2

238.93

-229.99

-157.24

-10.75

41.09

58.91

24.44

279.98

Oxygen

–

OH (aq) Phosphorus P( s,

white)

P 4(g) PH 3(g)

5.4

13.4

210.23

P 4O 10 (s )

-2984.0

-2697.0

228.86

H 3PO 3(aq)

-964.0

---

H 3PO 4(l)

-1266.9

–1111.69

---

Table A8-Inorganic Thermodynamic data at 25oC for assorted inorganic substances (continued). Substance

Enthalpy of formation 0 ∆ Hf

, kJ/mol

Free energy of formation 0 ∆ Gf ,

kJ/mol

Entropy 0

S , J/(K·mol)

H3PO4(aq)

-277.4

-1018.7

---

PCl3(l)

-319.7

-272.3

217.18

PCl3(g)

-287.0

-267.8

311.78

PCl5(g)

-374.9

-305.0

364.6

PCl5(s)

-443.5

---

K(s)

64.18

K(g)

89.24

60.59

160.34

K (aq)

-252.38

-283.27

102.5

KOH(s)

-424.76

-379.08

78.9

KOH(aq)

-482.37

-440.50

91.6

KF(s)

-567.27

-537.75

66.57

KCl(s)

-436.75

-409.14

82.59

KBr(s)

-393.80

-380.66

95.90

KI(s)

-327.90

-324.89

106.32

KClO3(s)

-397.73

-296.25

143.1

KClO4(s)

-432.75

-303.09

151.0

K2S(s)

-380.7

-364.0

105

K2S(aq)

-471.5

-480.7

190.4

18.83

-910.94

-856.64

41.84

42.55

Ag (aq)

105.58

77.11

72.68

Ag2O(s)

-31.05

-11.20

121.3

AgBr(s)

-100.37

-96.90

107.1

AgBr(aq)

-15.98

-26.86

155.2

AgCl(s)

-127.7

-109.79

96.2

AgCl(aq)

-61.58

-54.12

129.3

AgI(s)

-61.84

-66.19

115.5

AgI(aq)

50.38

25.52

184.1

-124.39

-33.41

140.92

Na(s)

51.21

Na(g)

107.32

76.76

153.71

Na (aq)

-240.12

-261.91

59.0

NaOH(s)

-425.61

-379.49

64.46

NaOH(aq)

-470.11

-419.15

48.1

Potassium

Silicon Si(s) SiO2(s,α) Silver Ag(s) +

AgNO3(s) Sodium

— Reference Tables 528 Appendix

Table A8-Inorganic Thermodynamic data at 25oC for assorted inorganic substances (continued). Substance

Enthalpy of formation 0 ∆ Hf

, kJ/mol

Free energy of formation 0 ∆ Gf ,

kJ/mol

Entropy 0

S , J/(K·mol)

NaCl(s)

-411.15

-384.12

72.13

NaBr(s)

-361.06

-348.98

86.82

NaI(s)

-287.78

-286.06

98.53

31.80

0.33

0.1

32.6

S (aq)

33.1

85.8

-14.6

SO2(g)

-296.83

-300.19

248.22

SO3(g)

-395.72

-371.06

256.76

H2SO4(l)

-813.99

-690.00

156.90

H2SO4(aq)

-909.27

-744.53

20.1

2–

SO4 (aq)

-909.27

-744.53

20.1

H2S(g)

-20.63

-33.56

205.79

H2S(aq)

-39.7

-27.83

121

SF6(g)

-1209

-1105.3

291.82

Sn(s, white)

51.55

Sn(s, gray)

-2.09

0.13

44.14

SnO(s)

-285.8

-256.9

56.5

SnO2(s)

-580.7

-519.6

52.3

Sulfur S(s, rhombic) S(s, monoclinic) 2–

Tin

Zinc Zn(s)

41.63

Zn (aq)

-153.89

-147.06

-112.1

ZnO(s)

-348.28

-318.30

43.64

— Reference Tables 530 Appendix

-1300 -1411 -1560 -2058 -2091 -2220 -2878 -3537 -3268 -3302 -3910 -3953 -3920 -3953 -5471

C2H2(g), acethylene

C2H4(g), ethylene

C2H6(g), ethane

C3H6(g), propylene

C3H6(g), cyclopropane

C3H8(g), propane

C4H10(g), butane

C5H12(g), pentane

C6H6(l), benzene

C6H6(g)

C7H8(l), toluene

C7H8(g)

C6H12(l), cyclohexane

C6H12(g)

C8H18(l), octane -726 -764 -1368 -1409 -3054

CH3OH(l), methanol

CH3OH(g)

C2H5OH(l), ethanol

C2H5OH(g)

C6H5OH(s), phenol

Alcohols, phenols

-890

∆ Hc , kJ/mol

Enthalpy of combustion

CH4(g), methane

Hydrocarbons

Substance , kJ/mol

-164.6

-235.10

-277.69

-200.66

-238.86

-249.9

---

-156.4

---

12.0

---

49.0

-146.44

-126.15

-103.85

53.30

20.42

-84.68

52.26

226.73

-74.81

0 ∆ Hf

Enthalpy of formation

Table A8-Organic Thermodynamic data at 25oC for assorted organic substances.

kJ/mol

-50.42

-168.49

-174.78

-161.96

-166.27

6.4

---

26.7

---

113.8

---

124.3

-8.20

-17.03

-23.49

104.45

62.78

-32.82

68.15

209.20

-50.72

0 ∆ Gf ,

Free energy of formation

Entropy

144.0

282.70

160.7

239.81

126.8

358

---

204.4

---

221.0

---

173.3

349

310.1

270.2

237.4

266.6

229.60

219.56

200.94

186.26

S , J/(K·mol)

-1166 -1192 -1790

CH3CHO (l), acetaldehyde

CH3CHO (g)

CH3COCH3 (l), acetone

-5645

C12H22O11 (s), sucrose -632 -3395 -969 -1085

CO(NH2)2 (s), urea

C6H5NH2 (l), aniline

NH2CH2COOH(s), glycine

CH3NH2 (g), methylamine

Nitrogen compounds

-2810

---

C6H12O6 (s), fructose

C6H12O6 (aq)

C6H12O6 (s), glucose

-2808

-3227

C6H5COOH (s), benzoic acid

Sugars

-254

(COOH)2 (s), oxalic acid

---

-875

CH3COOH (l), acetic acid

CH3COOH (aq)

-255

HCOOH (l), formic acid

Carboxylic acids

-571

∆ Hc , kJ/mol

Enthalpy of combustion

HCHO (g), formaldehyde

Aldehydes, ketones

Substance , kJ/mol

-22.97

-532.9

31.6

-333.51

-2222

-1266

---

-1268

-385.1

-827.2

-485.76

-484.5

-424.72

-248.1

-166.19

-192.30

-108.57

0 ∆ Hf

Enthalpy of formation kJ/mol

32.16

-373.4

149.1

-197.33

-1545

---

-917

-910

-245.3

-697.9

-396.46

-389.9

-361.35

-155.4

-128.86

-128.12

-102.53

0 ∆ Gf ,

Free energy of formation

Table A8-Inorganic Thermodynamic data at 25oC for assorted organic substances (continued). Entropy

243.41

103.51

191.3

104.60

360

---

212

167.6

120

86.6

159.8

128.95

200

250.3

160.2

218.77

S , J/(K·mol)