Chemistry dât tables

8/8/2019 Chemistry dt tables

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Appendix E

MHR 595

Appendix E

Table E.4 Conversion Factors

Quantity Relationships between units

length

mass

temperature

volume

pressure

energy

bp of H 2O = 373 .15 K (100 C)

1 m = 10 3 km

1 pm = 10 12 m

1 u = 1.66 10 27 kg

1 kg = 10 3 g

T (C) = T (K) 273.15

mp of H 2O = 273.15 K (0 C)

= 10 3 mL

1 mL = 1 cm3

= 10 3 g/mL= 1 g/L

1 J = 6.24 1018 eV

= 10 2 cm= 10 3 mm

= 10 3 t

0 K = 273.15 C

T (K) = T (C) + 273.15

= 10 3 m31 L = 1 dm 3

1 kg/m 3 = 10 3 g/m 3

= 760 mm Hg= 760 torr= 1 atm

101 325 Pa = 101.325 kPa

density

Chemistry Data TablesTable E.1 Useful Math Relationships

Table E.2 Fundamental Physical Constants (to sixsignicant digits)

Table E.3 Common SI Prexes

tera (T) 1012

giga (G) 109

mega (M) 106

kilo (k) 103

deci (d) 10 1

centi (c) 10 2

milli (m) 10 3

micro ( ) 10 6

nano (n) 10 9

pico (p) 10 12

9.806 65 m/s 2

6.022 14 1023/mol

9.109 38 10 31 kg

1.674 93 10 27 kg

1.672 62 10 27 kg

8.314 47 J/mol K

22.414 0 L/mol

2.997 92 108 m/s

1.660 54 10 27 kg

mass of electron ( m s)

mass of neutron ( m n)

mass of proton ( m p)

molar gas constant ( R

molar volume of gas at STPspeed of light in vacuo ( c

unified atomic mass ( u

acceleration due to gravity ( g

Avogadro constant ( N a)

charge on one mole ofelectrons (Faraday constant)

96 485.3 C/mol

)

)

)

)

D = mV

P =F

A

= 3.1416

Volume of sphere V = 43 r 3

Volume of cylinder = r2h


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596 MHR

Appendix E

Table E.6 Summary of Naming Rules for Ions

Table E.7 Summary of Naming Rules for Acids

Modern name ExampleClassical acid nameaqueoushydrogen ___ide

hydro___ic acid

HNO2, aqueoushydrogen nitriteor nitrous acid

HCl, aqueoushydrogen chlorideor hydrochloric acid

H2CO3, aqueoushydrogen carbonateor carbonic acid

___ic acid

___ous acidaqueoushydrogen ___ite

aqueoushydrogen ___ate

Type of ion ExamplePrefix or suffix

if the ion is the mostcommon oxoanion

-ate chlorate, ClO3

if the ion has the higherpossible charge

cuprous, Cu+

if the ion has one Oatom less than the mostcommon oxoanion

-ite

-ous

if the ion has two Oatoms less than the mostcommon oxoanion

if the ion has 1 Oatom more than themost common oxoanion

if the ion has 1 H atomadded to the mostcommon oxoanion

if the ion has 1 O atomless and 1 S atom morethan the most commonoxoanion

hypo-___-ite

per-___-ate

bi-

thio-

-ic

if the ion has the lowerpossible charge

chlorite, ClO2

hypochlorite,ClO

perchlorate,ClO4

bicarbonate,HCO3

thiosulphate,S2O32

titanic, Ti4+

Note: According to theStock system, metallicions are named usingRoman numerals.

The Romannumeral showsthe charge onthe metal ion

titanium(IV) Ti 4+copper(I), Cu+manganese(VII),

Mn 7 +

Polyatomic Ions

Metallic Ions

Table E.5 Alphabetical Listing of Common Polyatomic Ions

acetate

ammonium

arsenate

benzoate

borate

bromate

carbonate

Most common ion

CH3COO

NH4+

AsO 43

C6H5COO

BO33

BrO33

CO32

Common related ions

arsenite

tetraborate

AsO 33

B4O72

HCO3 bicarbonate

(hydrogencarbonate)

perchloratechloritehypochlorite

peroxide

iodide

nitrite

dichromate

cyanatethiocyanate

ClO4

ClO2

ClO

Cr2O72

glutamate

hydroxide

iodate

nitrate

oxalate

permanganate

phosphate

O2

2

I

NO2

OCN

SCN

C5H8NO4

OH

IO3

NO3

OOCCOO 2

MnO 4

PO43 phosphite

tripolyphosphate

ClO3chlorate

chromate

cyanide

CrO42

CN

PO33

P3O105

SO42sulfate

bisulfide(hydrogensulfide)

HSO4

SO32

HSO3

S2O32

bisulfate(hydrogensulfate)sulfite

bisulfite(hydrogensulfite)thiosulfate

S2sulfide HS

silicate

stearate

SiO32

C17H35COO

orthosilicate SiO44


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Appendix E

MHR 597

Table E.8 Standard Molar Enthalpies of Formation

Note: The enthalpy of formation of an element in itsstandard state is de ned as zero.

Table E.9 Ionization Constants for Acids

c o n t i n u e d

acetic acid

benzoic acid

chlorous acid

cyanic acid

formic acid

Acid Formula Conjugate base K a

CH3COOH

C6H5COOH

HClO 2HOCN

HCHO 2

HBr

CH3COO

C6H5COO

ClO2

OCN

CHO2

Br

1.8 10 5

6.3 105

1.1 10 2

3.5 10 4

1.8 10 4

1.0 109

1.3 106hydrochloricacid

hydrobromicacid

HCl Cl

hydrocyanicacid

hydrofluoricacid

hydrogen oxide

hypobromousacid

H2O

HOBr

HCN

HF

CN

OH

BrO

F

6.2 10 10

2.8 10 9

6.3 10 4

1.0 10 14

Al2O3(s)CaCO3(s)CaCl2(s)Ca(OH)2(s)CCl4( )CCl4(g)CHCl3( )CH4(g)C2H2(g)C2H4(g)C2H6(g)C3H8(g)C6H6( )CH3OH ( )

C2H5OH ( )CH3COOH ( )CO(g)CO2(g)COCl2(g)CS2( )CS2(g)CrCl3(s)Cu(NO 3)2(s)CuO (s)CuCl (s)

CuCl 2(s)

H

f(kJ/mol)Substance

1675.7 1207.6

795.4985.2128.2

95.7134.1

74.6+227.4

+ 52.4 84.0

103.8+ 49.1

239.2

277.6484.3110.5393.5219.1

+ 89.0+116.7556.5302.9157.3137.2

220.1

Substance

HBr(g)HCl(g)HF (g)HCN(g)H2O( )H2O(g)H2O2( )HNO 3( )H3PO4(s)H2S(g)H2SO4( )FeO (s)Fe2O3(s)Fe3O4(s)

FeCl 2(s)FeCl 3(s)FeS 2(s)PbCl 2(s)MgCl2(s)MgO(s)Mg(OH)2(s)HgS(s)NaCl (s)NaOH (s)Na2CO3(s)

36.3 92.3

273.3+ 135.1 285.8 241.8 187.8 174.1

1284.4 20.6

814.0 272.0 824.2

1118.4

341.8 399.5 178.2 359.4 641.3 601.6 924.5

58.2 411.2 425.6

1130.7

H

f(kJ/mol) Substance

NH3(g)N2H4( )NH4Cl(s)NH4NO3(s)NO(g)NO2(g)N2O(g)N2O4(g)PH3(g)PCl3(g)P4O6(s)P4O10(s)KBr(s)KCl(s)

KClO3(s)KOH(s)Ag2CO3(s)AgCl(s)AgNO 3(s)Ag2S(s)SF6(g)SO2(g)SO3(g)SnCl 2(s)SnCl 4( )

45.9+ 50.6

314.4365.6

+ 91.3+ 33.2+ 81.6+ 11.1

+ 5.4287.0

2144.3 2984.0

393.8436.5

397.7424.6505.8127.0124.4

32.6 1220.5

296.8395.7325.1511.3

H

f(kJ/mol)

Table E.10 Ionization Constants for Polyprotic Acids

Table E.11 Ionization Constants for Nitrogen Bases

1,2-diaminoethane(ethylenediamine)

Base FormulaConjugate

acid K b

dimethylamine(N-methylmeth-anamine)

NH2CH2CH2NH2 NH2CH2

(CH3)2NH

8.4 105

5.4 104(CH3)2NH2+

CH2NH3+

ethanamine

methanaminetrimethylamine(N-N-dimethyl-methanamine)

C2H5NH2

CH3NH2(CH3)3N

C2H5NH3+

CH3NH3+

(CH3)3NH+

4.5 104

4.6 104

6.4 105

ammonia

hydrazine

hydroxylamine

pyridine

aniline

urea

NH3N2H4NH2OH

C5H5N

C6H5NH2NH2CONH 2

NH4+

N2H5+

NH3OH+

C5H5NH+

C6H5NH3+

NH2CONH 3+

1.8 105

1.3 106

8.8 109

1.7 109

7.5 1010

1.3 1014

boric acid(aqueoushydrogen borate)

Acid Formula Conjugate base K a

5.4 10 10


4/5

598 MHR

Appendix E

Table E.12 Solubility Product Constants in Water at 25 C

Table E.13 Standard Reduction Potentials

c o n t i n u e d

F2(g) + 2e 2F (aq)

Co3+ (aq) + e Co2+ (aq)

H2O2(aq) + 2H+

(aq) + 2e 2H2O( )

Ce4+ (aq) + e Ce3+ (aq)

PbO 2(s) + 4H+

(aq) + SO42

(aq) + 2e PbSO 4(s) + H2O( )

MnO 4

(aq) + 8H+

(aq) + 5e Mn 2+ (aq) + 4 H2O( )

Au 3+ (aq) + 3e Au (s)

PbO 2(s) + 4H+

(aq) + 2e Pb2+ (aq) + 2H2O( )

Cl2(g) + 2e 2Cl (aq)Cr2O72

(aq) + 14H

+(aq) + 6e

2Cr3+ (aq) + 7H2O( )O2(g) + 4H

+(aq) + 4e

2H2O( )MnO 2(s) + 4H

+(aq) + 2e

Mn 2+ (aq) + 2 H2O( )IO3

(aq) + 6H

+(aq) + 6e

I (aq) + 3 H2O( )Br2( ) + 2e

2Br (aq)AuCl 4

(aq) + 3e

Au (s) + 4Cl

(aq)

NO3

(aq) + 4H+

(aq) + 3e NO (g) + 2 H2O( )

2Hg2+ (aq) + 2e Hg22

+(aq)

Reduction half reaction E

(V)

2.866

1.92

1.776

1.72

1.691

1.507

1.498

1.455

1.358

1.232

1.229

1.224

1.085

1.066

1.002

0.957

0.920

AgBrCuBr

PbBr 2

AgBrO 3TlBrO 3

Ag2CO3BaCO3CaCO3MgCO3PbCO 3

AgClCuCl

Ag2CrO4BaCrO4PbCrO

4

AgCNCuCN

BaF2CdF2CaF2FeF 2

Bromides

Carbonates

Chlorides

Chromates

Cyanides

Fluorides

5.38 10 51.10 10 4

5.35 10 136.27 10 9

6.60 10 6

8.46 10 122.58 10 93.36 10 96.82 10 67.40 1014

1.77 10 101.72 10 9

1.12 10 121.12 10 10

2.3 1013

5.97 10 173.47 10 20

1.84 10 76.44 10 33.45 10 112.36 10 6

4.01 10 9

6.47 10 6

1.14 107

1.12 10 10

AlPO 4Ca3(PO4)2Co3(PO4)2Cu3(PO4)2Ni3(PO4)2

Ba(IO3)2Ca(IO3)2Sr(IO 3)2Y(IO3)3

CuIPbI2AgI

1.27 10 129.8 10 9

8.52 10 17

9.84 10 212.07 10 332.05 10 351.40 10 374.74 10 32

BaSO4CaSO4Hg2SO4

1.08 10 104.93 10 5

6.5 10 7

CuSCNPd(SCN) 2

1.08 10 134.39 10 23

Iodides

Phosphates

Sulfates

Thiocyanates

Ca(OH)2Co(OH)2Eu(OH) 3Fe(OH) 2

Fe(OH) 3Pb(OH) 2Mg(OH)2Ni(OH) 2Sn(OH) 2Zn(OH) 2

5.02 10 65.92 10 159.38 10 274.87 10 17

2.79 103 9

1.43 10 205.61 10 125.48 10 165.45 10 27

3 10 17

Iodates

Hydroxides

Be(OH)2Cd(OH) 2

6.92 10 227.2 10 15

Bromates Ag+ (aq) + e Ag(s)

Hg22+

(aq) + 2e 2Hg( )

Fe3+ (aq) + e Fe2+ (aq)

O2(g) + 2H+

(aq) + 2e H2O2(aq)

I2(s) + 2e 2I (aq)

Cu+ (aq) + e Cu (s)O2(g) + 2H2O( ) + 4e

4OH (aq)Cu2+ (aq) + 2e

Cu (s)AgCl(s) + e

Ag(s) + Cl

(aq)

4H + (aq) + SO42

(aq) + 2e H2SO3(aq) + H2O( )

Cu2+ (aq) + e Cu + (aq)

2H + (aq) + 2e H2(g)

Fe3+ (aq) + 3e Fe (s)

Pb2+ (aq) + 2e Pb (s)

Sn 2+ (aq) + 2e Sn (s)

Ni2+ (aq) + 2e Ni (s)

Cd2+ (aq) + 2e Cd (s)Cr3+ (aq) + e

Cr2+ (aq)Fe2+ (aq) + 2e

Fe (s)Cr3+ (aq) + 3 e

Cr(s)Zn 2+ (aq) + 2e

Zn (s)2H2O( ) + 2e

H2(g) + 2OH

(aq)

Al3+ (aq) + 3e Al (s)

Mg2+ (aq) + 2e Mg(s)

La3+ (aq) + 3e La(s)

Na+ (aq) + e Na (s)

Ca2+ (aq) + 2e Ca(s)

Ba2+ (aq) + 2e Ba(s)

K+ (aq) + e K(s)

Li+ (aq) + e Li(s)

0.800

0.797

0.771

0.695

0.536

0.5210.401

0.342

0.222

0.172

0.153

0.000 0.037 0.126 0.138 0.257 0.403 0.407 0.447 0.744 0.762 0.828 1.662 2.372 2.379 2.711 2.868 2.912 2.931 3.040

Reduction half reaction E

(V)


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Appendix E

MHR 599

Table E.14 Speci c Heat Capacities of VariousSubstances

Table E.15 Average Bond Energies

c o n t i n u e d

HH

HC

HN

HO

HF

HSi

HP

HS

HCl

HBr

HI

HMg

436

338

339

460

570

299

297

344

432

366

298

126

Energy(kJ/mol)Bond

CC

CN

CO

CF

CSi

CP

CS

CCl

CBr

CI

347

305

358

552

305

264

259

397

280

209

Energy(kJ/mol)Bond

NN

NO

NF

NSi

NP

NS

NCl

NBr

NI

160

201

272

330

209

464

200

276

159

Energy(kJ/mol)Bond

PP

PS

PF

PCl

PBr

PI

SS

SF

SCl

SBr

SI

210

444

490

331

272

184

266

343

277

218

170

Energy(kJ/mol)Bond

Hydrogen Carbon NitrogenPhosphorusand sulfur

SubstanceSpecific heat capacity

(J/g C at 25 C)

aluminum

carbon (graphite)

copper

gold

hydrogen

iron

ammonia (liquid)

ethanol

water (solid)

water (liquid)

water (gas)

0.900

0.711

0.385

0.129

14.267

0.444

4.70

2.46

2.01

4.184

2.01

Element

Compound

Other material

air

concrete

glass

granite

wood

1.02

0.88

0.84

0.79

1.76

Note: The values in this table represent average valuesfor the dissociation of bonds between the pairs of atomslisted. The true values may vary for different molecules.

Table E.16 Average Bond Lengths

Note: The values in this table are average values. Thelength of a bond may be slightly different in differentmolecules, depending on the intramolecular forceswithin the molecules.

HH

HC

HN

HO

74

109

101

96

Length(pm)Bond

CC

CN

CO

CF

154

147

143

133

Length(pm)Bond

NN

NO

NF

NSi

146

144

139

172

Length(pm)Bond

PP

PS

PF

PCl

221

210

156

204

Length(pm)Bond

Hydrogen Carbon NitrogenPhosphorusand sulfur

HF

HSi

HP

HSHCl

HBr

HI

HMg

OO

OF

OSi

OP

OS

OCl

OBr

OI

92

148

142

134127

141

161

173

CSi

CP

CS

CClCBr

CI

186

187

181

177194

213

NP

NS

NCl

NBrNI

177

168

191

214222

PBr

PI

SS

SFSCl

SBr

SI

222

243

204

158201

225

234

148

142

161

160

151

164

172

194

SiSi

SiP

SiS

SiF

SiCl

SiBr

SiI

234

227

210

156

204

216

240

FCl

FBr

FI

ClBr

ClI

BrI

FF

ClCl

BrBr

II

166

178

187

214

243

248

143

199

228

266

C

C

C

N

N

O

C

C

C

N

134

127

123

122

120

121

121

115

113

110

Oxygen Silicon Halogens Multiple bonds

O

C

N

O

N

O

C

N

O

N

OO

OF

OSi

OP

OS

OCl

OBr

OI

204

222

368

351

265

269

235

249

SiSi

SiP

SiS

SiF

SiCl

SiBr

SiI

Si

226

364

226

553

381

368

293

640

FCl

FBr

FI

ClBr

ClI

BrI

FF

ClCl

Br Br

II

256

280

272

217

211

179

159

243

193

151

C

C

C

N

N

O

C

C

C

N

607

615

745

418

631

498

839

891

1077

945

Oxygen Silicon Halogens Multiple bonds

O

C

N

O

N

O

O

C

N

O

N

Energy(kJ/mol)Bond

Energy(kJ/mol)Bond

Energy(kJ/mol)Bond

Energy(kJ/mol)Bond

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