THE UNIVERSITY OF THE STATE OF NEW YORK Reference …

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THE UNIVERSITY OF THE STATE OF NEW YORK ? THE STATE EDUCATION DEPARTMENT ? ALBANY, NY 12234

Reference Tables for Physical Setting/CHEMISTRY

2011 Edition

Table A Standard Temperature and Pressure

Table D Selected Units

Name Standard Pressure

Standard Temperature

Value

101.3 kPa 1 atm

273 K 0?C

Unit

kilopascal atmosphere

kelvin degree Celsius

Table B Physical Constants for Water

Heat of Fusion Heat of Vaporization Specific Heat Capacity of H2O()

334 J/g 2260 J/g 4.18 J/g?K

Table C Selected Prefixes

Factor 103 10?1 10?2 10?3 10?6 10?9 10?12

Prefix kilodecicentimillimicronanopico-

Symbol k d c m n p

Symbol m g Pa K mol

J

s min h d y L ppm M

u

Name meter gram pascal kelvin mole

joule

second minute hour day year liter parts per million molarity

atomic mass unit

Quantity length mass pressure temperature amount of substance energy, work, quantity of heat time time time time time volume concentration solution concentration

atomic mass

Reference Tables for Physical Setting/ Chemistry ? 2011 Edition

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Table E Selected Polyatomic Ions

Formula

Name

H3O+

hydronium

Hg22+

mercury(I)

NH4+

ammonium

} CCH2H3C3OO2O? ? acetate

CN?

cyanide

CO32? HCO3?

carbonate

hydrogen carbonate

C2O42? ClO?

oxalate hypochlorite

ClO2? ClO3? ClO4?

chlorite chlorate perchlorate

Formula

Name

Cr O42? Cr2O72? MnO4? NO2? NO3? O22? OH?

chromate dichromate permanganate nitrite nitrate peroxide hydroxide

PO43? SCN?

SO32? SO42? HSO4? S2O32?

phosphate thiocyanate sulfite sulfate hydrogen sulfate thiosulfate

Table F Solubility Guidelines for Aqueous Solutions

Ions That Form Soluble Compounds

Group 1 ions (Li+, Na+, etc.) ammonium (NH4+) nitrate (NO3?) aCcHet3aCteO(OC?2)H3O2? or hydrogen carbonate (HCO3?) chlorate (ClO3?) halides (Cl?, Br?, I?)

sulfates (SO42?)

Exceptions

when combined with Ag+, Pb2+, or Hg22+ when combined with Ag+, Ca2+, Sr2+, Ba2+, or Pb2+

Ions That Form Insoluble Compounds*

Exceptions

carbonate (CO32?) chromate (CrO42?)

phosphate (PO43?) sulfide (S2?) hydroxide (OH?)

when combined with Group 1 ions or ammonium (NH4+) when combined with Group 1 ions, Ca2+, Mg2+, or ammonium (NH4+) when combined with Group 1 ions or ammonium (NH4+) when combined with Group 1 ions or ammonium (NH4+) when combined with Group 1 ions, Ca2+, Ba2+, Sr2+, or ammonium (NH4+)

*compounds having very low solubility in H2O

Reference Tables for Physical Setting/ Chemistry ? 2011 Edition

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Solubility (g solute/100. g H2O)

Table G Solubility Curves at Standard Pressure

150. KI

140.

NaNO3

130. KNO3

120.

110.

100.

90.

80. NH4Cl

70. HCl

60. KCl

50.

40.

NaCl

30. KClO3

20. NH3

10.

SO2

0

0

10. 20. 30. 40. 50. 60. 70. 80. 90. 100.

Temperature (?C)

Reference Tables for Physical Setting/ Chemistry ? 2011 Edition

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Vapor Pressure (kPa)

200. 150.

101.3 kPa 100.

Table H Vapor Pressure of Four Liquids

propanone ethanol

water

ethanoic acid

50.

0

0

25

50.

75

100.

125

Reference Tables for Physical Setting/ Chemistry ? 2011 Edition

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Table I Heats of Reaction at 101.3 kPa and 298 K

Table J Activity Series**

Reaction

CH4(g) + 2O2(g)

CO2(g) + 2H2O()

C3H8(g) + 5O2(g)

3CO2(g) + 4H2O()

2C8H18() + 25O2(g)

16CO2(g) + 18H2O()

2CH3OH() + 3O2(g)

2CO2(g) + 4H2O()

C2H5OH() + 3O2(g)

2CO2(g) + 3H2O()

C6H12O6(s) + 6O2(g)

6CO2(g) + 6H2O()

2CO(g) + O2(g)

2CO2(g)

C(s) + O2(g)

CO2(g)

4Al(s) + 3O2(g)

2Al2O3(s)

N2(g) + O2(g)

2NO(g)

N2(g) + 2O2(g)

2NO2(g)

2H2(g) + O2(g)

2H2O(g)

2H2(g) + O2(g)

2H2O()

N2(g) + 3H2(g)

2NH3(g)

2C(s) + 3H2(g)

C2H6(g)

2C(s) + 2H2(g)

C2H4(g)

2C(s) + H2(g)

C2H2(g)

H2(g) + I2(g)

2HI(g)

KNO3(s) H2O K+(aq) + NO3?(aq)

NaOH(s) H2O Na+(aq) + OH?(aq)

NH4Cl(s) H2O NH4+(aq) + Cl?(aq) NH4NO3(s) H2O NH4+(aq) + NO3?(aq) NaCl(s) H2O Na+(aq) + Cl?(aq)

LiBr(s) H2O Li+(aq) + Br?(aq)

H+(aq) + OH?(aq)

H2O()

H (kJ)* ?890.4 ?2219.2 ?10943 ?1452 ?1367 ?2804 ?566.0 ?393.5 ?3351 +182.6 +66.4 ?483.6 ?571.6 ?91.8 ?84.0 +52.4 +227.4 +53.0 +34.89 ?44.51 +14.78 +25.69 +3.88 ?48.83 ?55.8

*The H values are based on molar quantities represented in the equations. A minus sign indicates an exothermic reaction.

Most Active Least Active

Metals Li Rb K Cs Ba Sr Ca Na Mg Al Ti Mn Zn Cr Fe Co Ni Sn Pb H2 Cu Ag Au

Nonmetals Most Active

F2 Cl2 Br2 I2

Least Active

**Activity Series is based on the hydrogen standard. H2 is not a metal.

Reference Tables for Physical Setting/ Chemistry ? 2011 Edition

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