Lecture 5 Professor Hicks Inorganic Chemistry (CHE152) review - - PDF document

SLIDE 1

1

Lecture 5

Professor Hicks Inorganic Chemistry (CHE152)

Internal Energy (E)

system surroundings q heat released – (negative in sign) w work done by system

• (negative in sign)

q heat absorbed + (positive in sign) work done on system + (positive in sign)

change in internal energy E = q + w

like cash

• r

checks

review

examples of q and w

• inside a piston fuel burns

releasing heat and expanding pushing the piston up doing work

work absorbs heat +q makes surrounding cooler system releases heat -q

• a disposable first aid cold

pack does not change size much so work = 0, it absorbs heat when it is activated

system

review

SLIDE 2

2

Calculate the change in internal energy, E, when a system expands doing 155 J of work while absorbing 206 J of heat.

E = q + w absorbing heat adds energy to the system q = + 206 J doing work (expanding) removes E from system w = –155 J E = 206 J -155 J = 51 J

system surroundings q heat absorbed by system + (positive in sign) +206 J w work done by system

• (negative in sign)
• 155 J

review

Enthalpy (H)

• heat released under constant pressure =

enthalpy change (H)

• Constant pressure
• Conditions for reactions of life
• Conditions of most chemical reaction unless

they are run in constant volume containers

• only reflects part of the internal energy change

since it is the heat only not the work

• the alternative to constant pressure is constant

volume like the aging of wine in a glass bottle

review system surroundings C6H12O6 (g) + 6O2 (g)  work heat

Enthalpy is heat released under constant pressure

6CO2 (g) + 6H2O (g) change in enthalpy H = q change in internal energy E = q + w review

SLIDE 3

3

First law of thermodynamics

kinetic energy potential energy heat applied when energy changes forms energy like a liquid energy cannot be created or destroyed Rudolf Clausius review

When things go downhill…

A 10 kg bowling ball at a height of 100 m has potential energy due to gravity Potential energy = mgh = 10 kg x 9.8 m/s2 x10 m = 9800 J As it falls it speeds up converting potential energy into kinetic energy Right before it hits ground all the potential energy has become kinetic energy = 9800 J After it hits the ground it is not moving so kinetic energy is zero- all the energy has become heat = 9800 J Heat 9800 J review potential energy

Energy changes forms

(but does not get destroyed)

1) potential energy = 9800 J 2) kinetic energy = 9800 J 3) heat 9800 J heat kinetic energy as ball falls PE  KE 9800 J 9800 J 9800 J

• n

impact KE  heat atmospheric P is constant so heat = H = -9800 J review

SLIDE 4

4

First law and chemical reactions

• If a process is reversed an equal amount of

energy must be exchanged in the opposite direction H and E have the opposite sign

• H and E depend upon the amount of material

reacted so doubling, tripling reaction doubles, triples etc. the H and E

• For a multistep process simply add up each steps

H and E to get overall value (Hess’ Law) For a cyclic process H and E = 0

First law and chemical reactions

• Example: Determine the Ho for

2CO2 (g)  2C (s) + 2O2 (g) given that C (s) + O2 (g)  CO2 (g) Ho = - 393 kJ

Ho = 2 x 393 kJ = 786 kJ

review

Hess’ law

SLIDE 5

5

Second Law

• Heat only flows from

hotter to cooler

• Explains why processes

that release heat tend to not reverse themselves

Sadi Carnot

Second law

• Simplest way to state the second law (and it

works for most cases) is “Heat only flows from hotter to cooler”

• the second law explains why processes that

release heat do not spontaneously reverse themselves

HOT COLD q (heat) BOTH SAME TEMPERATURE heat will not flow between objects at same temperature

SLIDE 6

6

Second Law

heat 9800 J

bowling ball is trapped (bonded) to the earth because it has lost the energy it would need to go back to the top of building when the ball hit the ground and the energy becomes heat the ball warms up a little.

system surroundings hotter cooler system surroundings same temperature

Second law and chemical reactions

• chemical reactions absorb/release heat
• Obeying second law leaves them stuck at

lowest energy like the bowling ball

CH4 (g) + 2O2 (g)  CO2 (g) + 2H2O (g) + heat CH4 (g) + 2O2 (g)  CO2 (g) + 2H2O (g) + heat

hotter cooler

 CO2 (g) + 2H2O (g)

system surroundings same temperature system surroundings heat is like a limiting reagent for reverse reaction

Fuels

CO2 + H2O

have chemical potential energy new compounds with less chemical potential energy Sometimes some Is used to do work the rest comes

• ut as heat

First law says the fuels cannot be recovered without putting energy back in Second law says the energy that has left as heat will not flow back because heat will only flow from hotter to cooler

SLIDE 7

7

The Standard State

• to be able to compare reactions a

standard state for every elements is defined

• all substances at concentration of 1.0 M

gases at a partial pressure of 1.0 atm

• Standard Enthalpy Change (Ho)

Standard Formation Reactions

• form 1 mole of a substance from elements

in most stable state

• most elements just element solids
• some elements exist as diatomic gases

F2, Cl2, N2, O2, H2

• Br2 and Hg liquid and I2 is a solid
• Standard Enthalpy for this reaction is

called standard enthalpy of formation Ho

f

Standard Formation Reactions

• Example: a) Write standard formation

reactions for CO2 (g), H2O (l), C8H18 (l), and CHCl3 (l).

• 8C (s) + 9H2 (g)  C8H18 (l)
• C(s) + 3/2 Cl2 (g) + ½H2 (g)  CHCl3 (l)
• C (s) + O2 (g)  CO2 (g)
• H2 (g) + ½ O2 (g)  H2O (l)

Ho

f

Use the Standard Formation Reaction Data Tables to determine H for these reactions

SLIDE 8

8

See tables full size appended to the end of the lecture packet

Elements in the standard state

substance A substance B Ho = ? elements in standard state +enthalpy formation for B  Ho

f (B)

• enthalpy formation for A
• Ho

f (A)

standard state is like a train junction where you transfer for your final destination

home station destination junction

• Ho

f (A) + Ho f (B)

Hess’ Law

CH4(g) + 2O2(g)  CO2(g) + 2H2O(g) Ho = ?

elements in standard state

• Hof (CH4)

+

• Hof (O2) x 2

+Hof (CO2) + +Hof (H2O) x 2

Ho = npHo

f - nrHo f

reaction

SLIDE 9

9

See tables full size appended to the end of the lecture packet

Hess’ Law

CH4(g) + 2O2(g)  CO2(g) + 2H2O(g) Ho = ?

elements in standard state

• Hof (CH4)
• Hof (O2) x 2

Hof (CO2) Hof (H2O) x 2

• 802.5 kJ

Ho = 1 x (-393.5) + 2 x (-241.8) - (1 x - 74.6 + 2 x 0) = products - reactants npHo

f - nrHo f

Ho = npHof - nrHof

reaction

6CO2 (g) + 6H2O (g) 6CO (g) + 6H2O (g) + 3O2 (g) Ho3 C6H12O6 (s) + 6 O2 (g) 3C2H2 (g) + 3H2O2 (l) + 6O2 (g) 6C (g) + 18O (g) + 12H (g) Ho2 Ho1 Ho4 Ho5 Ho6 Ho8 Ho7

Form groups of two or three. Every group is assigned one reaction for which to find Ho

SLIDE 10

10

Entropy

Ludwig Boltzmann

• Entropy (S)
• imaginary substance
• associated with disorder
• matter or energy spreads out

 entropy increases

• Standard Entropy Change (So)

entropy (disorder)

• In a chemical reaction the side that

has more moles of gas has more entropy A (solid)  B(gas) Entropy increases S positive

• The side that has a material

dissolved in a solvent has more entropy

A (solid)  A (aqueous) entropy increases so S positive

Is S positive or negative ?

2C8H18(g) +25O2(g) 16CO2(g) + 18H2O (g) 27 moles gas 34 moles gas (less moles gas) (more moles gas)

Under constant pressure and temperature more moles gas will have to occupy larger volume And is therefore more spread out

Change in entropy S = Sfinal – Sinitial more – less + positive +

V = nRT P



n



V (less entropy) (more entropy)

SLIDE 11

11

Entropy is created when heat flows from hotter to cooler

• S > q/T
• T must be in Kelvins
• Processes where entropy is created are said

to be Irreversible

• Irreversible does not mean they can never

be reversed, but rather that energy will have to be added to reverse it

• The most precise way to state the second

law is “In any spontaneous process the entropy of the universe increases” Example: Estimate the entropy created when 1000 Joules of heat flows from a Bunsen burner flame at 600 C into a boiling water bath at 100 C. Example: When heat is absorbed by boiling water the temperature does not

• rise. The energy is used to turn liquid

water into steam which contains the added

• energy. If the system is taken to be the

liquid and gaseous water, how much entropy is created when 1 mole of liquid water undergoes evaporation?

SLIDE 12

12

Entropy and Spontaneity

• Processes that have positive S values

tend to not reverse themselves

• The more matter spreads the lower its

concentration/partial pressure

• From a kinetic standpoint reverse reaction

is slower and slower…

H2O (l) + CO2 (g) H2SO4 (aq) + Na2CO3 (aq)

Gibbs Free Energy

Both should be visualized as products forming that escape preventing reaction from reversing

Josiah Willard Gibbs

two reasons a process can be spontaneous: 1) heat released (H negative) 2) matter spreads out (S positive)

system

• q

system +S

G H S

SLIDE 13

13

Gibbs Free Energy (G)

Gibbs free energy expresses both factors that affect if a reaction will happen H and S G = H-TS

• G is negative = thermodynamically spontaneous
• accounts for heat and entropy
• G is the theoretical maximum amount of work that can be
• btained

Why did Gibbs makes a negative G spontaneous?

reaction quotient (Q) negative sign = spontaneous picked to be like gravity G like height so G negative like falling to lower height graph of G is always shaped like a bowl if  G= negative the system sits on the walls of a bowl on reactant side if  G = positive the system sits on the walls of a bowl on product side G

“Thermodynamically spontaneous”

• does NOT mean happens fast or slow
• if it is thermodynamically spontaneous then

it CAN HAPPEN and if it does it will tend to not reverse itself

• if it can happen, kinetics tells how

FAST/SLOW

SLIDE 14

14

Standard Gibbs Free Energy (Go)

If measured under standard conditions Go = Ho-TSo

• Ho and So can be calculated from

standard formation values

• Go calculated at any temperature

Ho and So do not change much with temperature

Example: If a reaction has Ho = +1255 kJ/mol and So = 4.0 kJ/mol*K at 300 K. a) Calculate Go at 1.0 K. b) Calculate Go at 300 K. c) How high must the temperature be raised in order for the reaction to become thermodynamically spontaneous by 1 kJ/mol?

a) Go = Ho-TSo Go = +1255 – 1.0 * 4.0 (kJ/mol) K * (kJ/mol*K) = (1255 – 4) kJ/mol = +1251 kJ/mol b) Go = Ho-TSo Go = +1255 – 300 * 4.0 (kJ/mol) K * (kJ/mol*K) = (1255 – 1200) kJ/mol = +55 kJ/mol c) Go = Ho-TSo

• 1 = +1255 – T * 4.0

(kJ/mol) K * (kJ/mol*K) T*4.0 = +1256 T = 1256/4 = 314 K

positive = not spontaneous positive = not spontaneous

Go Temp Dependent (an example)

negative negative positive Fe2O3 (rust) 3Fe (s) + 2 O2 (g)  Fe3O4 (s) + heat a) Is So positive or negative? b) Is Ho positive or negative? c) At high temperature is Go positive or negative?

Fe (metal)

O2 O2 O2 O2

heat

high temp reverse reaction becomes spontaneous as the forward reaction become non-spontaneous metal oxidized

SLIDE 15

15

State Functions

• Properties that only depend on the final

and initial conditions are said to be state functions

• How far you are from home is a state

function

• How far you may have traveled is not a

state function

• E, H, S, and G are all state functions

State Functions

• Because E, H, S, and G are all state

functions their overall value must be zero for a cyclic process

6CO2 (g) + 6H2O (g) 6CO (g) + 6H2O (g) + 3O2 (g) So4 C6H12O6 (s) + 6 O2 (g) 3C2H2 (g) + 3H2O2 (l) + 6O2 (g) 6C (g) + 18O (g) + 12H (g) So2 So1 So5 So3 Cycle adds up to zero!!! Entropy may have been created outside the system to cause the cycle to happen but for the atoms that underwent it (the system) the S was zero

SLIDE 16

16

Example: Can more work be obtained from burning a gallon of octane if it is burned at constant pressure or constant volume?

SLIDE 17

17

SLIDE 18

18

Example: If the H for the reaction A + B  C is +500 kJ/mol and S is -300 J/mol*K calculate G at 25 C Does C form spontaneously from A+B? Is there a temperature G where = 0?

SLIDE 19

w

".,i- ",;' ':

• .-'

.; ' '.i.

I : - - t : ' t l , ' - : r - l * : :

;i- .rj- ,* ]1**" 1--' 1o* "i,- ,',,.,.,-.,i*

A. Atomic Golors

Atomic number: Atomic symbol: Atomic number: Atomic symbol: Atomic number: Atomic symbol:

B. Standard Thermodynamic Guantities for Selected Substances at e5 "C

4

W

Be

1 2

@

Mg 29

@

rw

v

Cu 1

#

H 1 l

ffim

ffi

v Na

20

ffi

Ca 1 9

W

K

8

IUtsTL E E w

• @

CI

7

ffi

N

6 ^-. E

r

• C

1 5

m mrmn w Ev

P 5

ffi

W

B 30

@

Zn

AHi (kJlmol) AGi (kJlmol) S'(J/mol . K)

35

• L

E

xsm

E E wUZ

Br 53

@

w w

• I

Substance

Aluminum Al(s)

Al(s)

rt13+(aq) AlC13(s) A1203(s) Barium Ba(s) Ba(g) Ba?+(aq) BaC03(s) BaCl2(s) Ba0(s) Ba(0H)2(s)

330.0

• 538.4
• 704.2
• t675.7

i80.0

• 537.6
• t213.0
• 855.0
• s48.0
• 944.7

289.4

• 483
• 628.8
• 1582.3

146.0

• 560.8
• n34.4
• 806.7
• 520.3

28.32 t64.6

• 325

109.3 50.9 62.5 t70.2 9.6 r12.l 123.7 72.1

Substance BaS0a(s) Beryllium Be(s) Be0(s) Be(0H)u (s) Bismuth Bi(s) BiCl3(s) Bi203(s) Bi2S3(s) Boron B(s)

B(s)

AHi ftJ/mol)

• t473.2
• 609.4
• 902.5
• 379.1
• 573.9
• i43.

i 565.0 AGf (kJ/mol) S" (j/mol .K)

• t362.2

132.2 9.5

• 580.1

13.8

• 815.0

45.5 56.7

• 315.0

177.0

• 493.7

151.-5

• 140.6

200.4 5.9 521.0 153.4 (continued

• n

the next page)

I 6

A-7

SLIDE 20

A.B

A P P E N D I X I I : U S E F U L DATA

AGi (kJlmot)

• 388.7
• 1119.4

87.{',

• 1194.3
• 968.9

82.4 3.1

• 102.8
• 53.4

77.3

• 77.6
• 343.9
• 228.7
• 156.5
• 822.7

144.0

• 553.6
• 64.9
• 1129.1
• 748.8
• 117-5.tr
• t42.s
• 742.8
• 603.3
• 897.5
• 1322.0
• 3884.7

2.9 671.3

• -50.5
• 60.2
• o).t
• 73.7
• 62.3
• 66.4
• 102.5
• 361.4

32.7 * 166.6

• 162.3

209.9 68.4

Substance BCl3fu)

BF:(g) BzHok) 8203(s) H3803(s) Bromine Br(g) Br2(/)

Brzk)

Br-(aq) HBr(g) Cadmium Cd(s) cd(g) cdz+(aq) CdClz(s) Cd0(s) CdS(s) CdS0+(s) Calcium Ca(s) ca(g) ^ )+, La- \aq) CaC2(s) CaC03(s) CaCl2(s) CaF2(s) CaH2(s) Ca(N03)2(s) Ca0(s) Ca(0H):(s) CaS0a(s) Ca3(P0a)2(s) Carbon C(s, graphite) C(s, diamond)

c(g) cH+(g)

CH3CI(g) cH2cl2Q) cH2cl2(/) . cHCl3(/) CCI+(g) ccl4(/) CH20(g) CH202(1, fonnic acid) CH3NH2(g, methylamine) cH30H(/) CH30H(g) CzHzk) czH+(g)

AHi (kJ/mol)

• 403.8
• i

136.0

1 / I

JO.+

• t273.5
• 1094.3

I 1 1 . 9 30.9

• 1 ) 1 4
• 36.3

1 1 1 . 8

• 75.9
• 391.5
• 258.4
• 161.9
• 933.3

177.8

• 542.8
• 59.8
• t207.6
• 7q\ 4
• 1228.0
• 1 8 1 . 5
• 938.2
• 634.9
• 985.2
• 1434.5
• 4120.8

I.BB 716.7

• 7 4.6
• 8 r . 9
• 95.4
• 1 ' l A 1

L L A . L

• 134.1
• 95.7
• 128.2
• 108.6
• 425.0
• 22.5
• 238.6
• 201.0

))'7 4

52.4

S'(J/mot.K)

?q0 I

254.4 232.1 54.0 90.0 ' 175.0 r52.2 245.5 80.71 198.7 51.8 167.7

• 73.2

I 1 5 . 3 54.8 64.9 123.0

+ I . O

t54.9 *53.1 70.0 9r.7 108.4 68.5 41.4 193.2 38. l 83.4 106.5 236.0 5.7

) 4

158.1 r 86.3 234.6 270.2 177.8 201.7 309.7 216.4 218.8 129.0 242.9 126.8 239.9 200.9 219.3

Substance CzHok) c2H-50H(/)

C2H5OH(g)

C2H3Cl(g vinyl chloride) C zH 4clz(1, di chl

• ro

e th an e ) C2Ha0(g acetaldehyde) C1H4OzQ, acetic acid) C:Hsk) CaH60(/, acetone) C3H70H(i, isopropanol ) c+Hro(/) CaHrok) coHe(/) C6H5NH2(/, aniline) C6H50H(s, phenol) C6H1206(s, glucose) csHr8(/) C16Hs(s, naphthalene) C12H22011(s, sucrose)

AHi (kJ/mot) AGi (kJi mot) S" (Umot.K) co(g) cozk)

co2@q)

co?-tuq)

HCol(aq) H2cQ@q) CN-(a4) HCN(/) HCN(g)

csz(/) CSzk) c0cr2fu)

C,;o(s)

C"rium

Cs(s) cs(g)

^ + , Ls \aq) CsBr(s) CsCI(s) CsF(s) Csl(s) Chlorine cl(g)

clzk) Ct-(aq)

HCI(g) HCt(aq) clo2Q) Cl2o(g) Chromium Cr(s)

c(g)

Cr3+(aq)

• 84.68
• 277.6
• 234.8

) / . L

• 166.8
• 166.2
• 484.3
• 103.85
• 248.4
• 318.

r

• 1 4 7 7
• r25.7

49.1 3t.6

• 165.r
• 1273.3
• 250.I

78.5

• 2226.1
• 1r0.5
• 393.5
• 413.8
• 677

.r

• 692.0
• 699.7

1 5 1 108.9 i35. r 89.0 116.7

• 219.r

2327.0 76.5

• 258.0
• 400
• 438
• 553.5
• 32.0
• 174.8
• 167

.9 53.6

• 79.6
• 133.0
• 389.9
• 155.6
• 15.0
• 15.71

124.5 149.2

• 50.4
• 910.4

201.6

• 1544.3
• r37.2
• 394.4
• 386.0
• 527.8
• 586.8
• 623.2

r66 125.0

t ) 4 7

64.6 67.1

• 204.9

2302.0 49.6

• 292.0
• 387
• 414
• 525.5
• 337

105.3

• t3t.2
• 95.3
• r3t.2

120.5

97.9 351.8

229.2 160.7 281.6 264.0 208.5 263.8 159.8 270.3 199.8 1 8 1 . 1 231.0 310.0 173.4 191.9 144.0

1 1 1 1 a t L . l

t67.4 360.24 197.7

z 1 ) . 6 1 t / . 6

• s6.9

9r.2

t87.4 1 1 8 112.8 201.8 1 5 1 . 3 237.8 283.5 426.0 85.2 175.6 t32.1 t17 101.2 92.8

r27

165.2

223.r

)o.o 186.9 50.)

/50.d, too.L

23.8 t74.5

I / . t . J

• t67

.l

• 92.3
• 167

.2 t02.5 80.3 396.6

• r971

SLIDE 21

A P P E N D I X I I : U S E F U L D A T A

A-9

Substance

cro]-tuq)

C1203(s)

Cr2ol-fuq)

Cobalt Co(s) co(g) Co0(s) Co(0H)z(s) Copper Cu(s) cu(g)

^ + l

LU \aq) ^ )+/ Lv- taq) CuCl(s) CuCl2(s) CuO(s) CuS(s) CuS0q(s) Cu20(s) Cu2S(s) Fluorine F(g) Fzk) F-(aq) HF(g) Gold Au(s) Au(g) Helium He(g) Ilydrogen H(g)

u*(aq)

H-(g)

ulki

Iodine I(g) Iz(s)

Izk) r-(aq)

HI(g) Iron Fe(s) Fe(g) Fez+ (aq) Fer+(aq) FeC03(s) FeCl2(s) FeClj(s) AHi (kJlmol)

• 872.2
• 1139.7
• 1476

424.7

• 237.9
• 539.7

337.4 5 1 . 9 64.9

• r37.2
• 220.1
• t57

.3

• 53.1
• 7 7 1 4
• 168.6
• 79.5

79.38

• 335.35
• 273.3

366. l 2 iB.0 1536.3 106.76 62.42

• 56.78

26.5 4t6.3

• 87.9
• 47.69
• 740.6
• 341.8
• 399.5

AGi (kJlmol)

• 717.r
• 1058.1
• 1279

380.3

1 r / a

• L r+.^/.
• 454.3

297.7 50.2 65.5

• I19.9
• 175.7
• t29.7
• 53.6
• 662.2
• 146.0
• 86.2

/ ^ a

OL.J

• 278.8
• ) 7 \ 4

326.3 203.3 l5 17, I 70.2 19.3

• 5t.57

r.7

370.7

• 84.94
• 10.54
• 666.7
• 302.3
• 334.0

S" (J/mol .K)

44 81.2 238 30.0 179.5 53.0 79.0 33.2 166.4

• 26
• 98

86.2 108. I 42.6 66.5 r09.2 93.1 r20.9 158.75 202.79

• 13.8

173.8 47.4 180.5 t26.2 t14.7 108.9 t30.7 r80.79 I 16.14 260.69 106.45 206.6

L / . )

180.5 113.4 293.3 92.9 1 1 8 . 0 142.3 Substance Fe0(s) Fe(0H):(s) FeS2(s) Fe203(s) Fe30a(s) Lead Pb(s) Pb(g) vbz+(aq) PbB12(s) PbC0:(s) PbCl2(s) Pbl2(s) Pb(N0:)z(s) Pb0(s) PbOz(s) PbS(s) PbS0a(s) Lithium Li(s) Li(g) Lt+(aq) LiBr(s) LiCl(s) LiF(s) Lil(s) LiNO3(s) Li0H(s) Li20(s) Magnesium Mg(s) Mg(g) tttg2+ (a4) MSCI2(s) MgC03(s) VIgF2(s) MgO(s) Mg(0H)2(s) MgS0a(s) lvl93N2(s) Manganese Mn(s) Mn(g) Mn2+(aq) NIn0(s) Mn02(s) Mn0f(aq) Mercury

Hs(/) Hsk)

AHi (kJlmol)

• 272.0
• 823.0
• t78.2
• 824.2
• 1 1 1 8 , 4

r95.2 0.92

• 278.7
• 699.r
• 359.4
• 175.5
• 45

r.9

• 2t7.3
• 277.4
• 100.4
• 920.0

159,3

• 278.47
• 351.2
• 408.6
• 616.0
• 270.4
• 483.

r

• 487.5
• 597.9

147.1

• 467.0
• 64t.3
• 1095.8
• 1124.2
• 601.6
• 924.5
• t284.9
• 461

280.7

• 2r9.4
• 385.2
• 520.0
• 529.9

6 1 . 4 AGf (kJlmol) S'(J/mol . K)

• 255.2

64.75

• 696.5

106.7

• 166.9

52.9

• 742.2

87.4

• 1015.4

t46.4 162.2

• 24.4
• 26t.9
• 625.5
• 3 1 4 . 1
• r73.6

64.8 175.4 18.5 161.5 1 3 1 . 0 136.0 t74.9 * r87 .9 68.7

• 2173

68.6

• 98.7

9r.2

• 813.0

148.5 29.r 126.6 138.8

• 293.3

t2.24

• 342.0

74.3

• 384.4

5.9.3

• 587.7

35.7

• 270.3

86.8

• 381.1

90.0

• 4415

42.8

• 561.2

37 .6 32.7 rr2.5 148.6

• 455.4
• 137
• 591.8

89.6

• 1012.1

65.7

• 1071.1

57 .2

• 569.3

27.0

• 833.5

63.2

• 1170.6

9r.6

• 401

88 32.0 238.5 173.7

• 22s.6
• 78.8
• 362.9

59.7

• 465.1

53.1

• 436.2

190.6 75.9 31.8 175.0 (continuetl

• n

the next page)

SLIDE 22

A-10

Substance tlg2+(aq)

) + ,

n9z- \a4) HgCl2(s) HgO(s) HgS(s) H92Cl2(s) Nickel Ni(s) Ni(g) NiCl2(s) Ni0(s) NiS(s) Nitrogen N(g) Nz(g) NF:(g) NHik) NH3(c4) Nun+(aq) NHaBr(s) NHaCI(s) NHaCN(s) NHaF(s) NHaHC0j(s) NHal(s) NHaNO3(s) NHaN03(a4) HN0rk) HN03(a4) No(g)

Nozk)

N03 (aq)

N0Br(g) N0cl(g) NzH+(/) NzHak) Nzo(g) Nzo+(/) Nzo+(g)

N205(s)

Nzosk) Orygen

• (s)
• z(g)
• :(g)

OH-(aq) Hzo(/) Hzo(g) H202(/) H:ozk)

AHi (kJlmol)

170.21 166.87

a a / a

• /z+.J
• 90.8
• 58.2
• 265.4

429.7

• 305.3
• 239.7
• 82.0

472.7

• 1 3 2 . 1
• 45.9
• 80.29
• 133.26
• 270.8
• 314.4

0.4

• 464.0
• 849.4
• 201.4
• 365.6
• 339.9
• 133.9
• 207

9r.3

33.2

• 206.8s

82.2 51.7 s0.6 95.4 8 1 . 6

• 19.5

I l . t

• 43.1

I J.J

249.2 142.7

• 230.02
• 285.8
• 24r.8
• 187.8
• 136.3

AGf (kJlmol)

164.4 153.5

• 178.6
• 58.5
• 50.6
• 2r0.7

384.5

• 259.0
• 2 n . 7
• 79.5

455.5

• 90.6
• t6.4
• 26.50
• 79.3r
• 175.2
• 202.9
• 348.7
• 665.9
• 112.5
• 183.9
• 190.6
• 73.5
• 110.9

87.6 5 1.3

• i 10.2

, 82.4 66. I r49.3 t59.4

r03.7

97.5 99.8 113.9 n7.I 231.7 163.2

• 157

.3

• 237.r
• 228.6
• 120.4
• 105.6

S" (J/mol .K)

• 36.19

65.74 146.0 70.3 82.4 191.6 29.9

r82.2

97.7 37.99 53.0 153.3 1 9 1 . 6 260.8 192.8 i 1 1 . 3 r1t.I7 113.0 g/,.6 72.0

1 l n

• I

17.0 l5 1.1 259.8 266.9 r46 210.8 240.1 t46.70 273.7 26r.7

r2r.2

238.5 220.0 209.2 304.4 178.2 355.7 l 6 t . t 205.2 238.9

• 10.90

70.0 188.8. 109.6 232.7 Substance Phosphorus P(s, white) P(s, red) P(g) PzQ) P+(g) PCI3(/) PClrk) PCls(s) PCl5ft) PFsk) PHrk) P0c]3(/) P0Clj(g)

Pof-tuq) HPof-@q)

H2POa @q) H3P0a(s) \Poa@q) Pa06(s) Pa016(s) Platinum Pt(s)

Pt(s)

Potassium I((s)

K(s)

x*(aq) KBr(s) I(CN(s) KCI(s) KCl0r(s) KCi0a(s) KF(s) Ifl(s) KN03(s) K0H(s) KoH(aq) K02(s) K2C03(s) K20(s) K202(s) K2S0a(s) Rubidium Rb(s) Rb(g) Rb+(aq) RbBr(s) RbCl(s) RbClO3(s)

AHi fiJlmol)

• r7.6

316.5 r44.0 58.9

• 319.7
• 287.0
• 443.5
• 374.9
• 1594.4

5.4

• 597.1
• 558.5

1 ^ - - '

• t / / t u
• 1292.r
• t296.3
• 1284.4
• 1288.3
• 1640.1
• 2984

56s.3 89.0

L J L . L 1

• 393.8
• I13.0
• 436.5
• 397.7
• 432.8
• 567.3
• 327.9
• 494.6
• 424.6
• 482.4
• 284.9
• 1 1 5 1 . 0
• 36r.5
• 494.1
• 1437.8

80.9

• 25r.12
• 394.6
• 435.4
• 392.4

AGi (kJlmol)

• 1 2 . 1

280.1 103.5 24.4

• 272.3
• 267.8
• 305.0
• 1520.7

13.5

• 520.8
• 512.9
• 1018.7
• 1089.2
• t130.2
• t124.3
• 1142.6
• 2698

U

520.5 60.5

• 283.3
• 380.7
• 101

.9

• 408.5
• 296.3
• 303.

r

• 537.8
• 324.9
• 394.9
• 379.4
• 440.5
• 239.4
• r063.5
• 322.1
• 4) \

1

• 1321.4

53. r

• 283.1
• 381

.8

• 407.8
• 292.0

S" (j/mot.(y

4 1 . 1 22.8 163.2 2 l8.l 280.0 2r7.1 3 1 1 . 8 364.6 300.8

) 1 n )

1 a . F

325.5

• ) ? n c
• . ) ' l ' r

90.4 I10.5 158.2 228.9 41.6 192.4 64.7 160.3 101.2 95.9 128.5 82.6 143.1 r 51.0 66,6 106.3

I J J . I

8r.2

91.6 n6.7 155.5 94.14

102.r

t75.6 76.8 170.1

rzt.75

110.0 95.9 152 A P P E N D I X I I : U S E F U L D A T A

''"rt:, ,*, i'

SLIDE 23

A P P E N D I X l l : U S E F U L D A T A A - 1 1

AHiftJ/mol) AGi (kJlmol) S'(J/mol' K)

Substance RbF(s) Rbi(s) Scandium Sc(s) sc(g) Selenium Se(s, gray) se(g) H2Se(g) Silicon Si(s)

si(s)

sicl4(/) SiFa(g) siHaQ) Si02(s, quartz) si2H6Q) Silver Ag(s)

Ag(s)

. + ,

Lg'\aq) AgBr(s) AgCl(s) AgF(s) Agl(s) AgNO3(s) Ag20(s) Ag2S(s) Ag2S0a(s) Sodium Na(s) Na(g) Na-(a4) NaBr(s)

Ndct(s)

NaCl(ar1) NaCl03(s) NaF(s) NaHC0:(s) NaHS0a(s) Nal(s) NaN0:(s) NaN03(aq) NaOH(s) NaOH(aq) NaO2(s) Na2C03(s) Na20(s) Na202(s)

Substance

Na2S0a(s) Na3P0a(s) Strontium Sr(s) Sr(g)

s4+@q)

SrCl2(s)

srior(s) Sr0(s)

SrS0a(s) Sulfur S(s, rhombic) S(s, monoclinic)

s(g) szk)

Ssk) s2-(oq) sFok) HS-(aq) Hzs(g) H2S(aq) socl2(/)

sozk) sor(g) s0f-(aq) HS0f(a4)

H2So4(/) H2SO4@q)

svol-bq)

Tin Sn(s, white) Sn(s, gray) sn(g) SnCl+(/) SnCI+(g) Sn0(s) Sn02(s) Titanium Ti(s)

ri(g) ric14(i) ricLk)

Ti02(s) Tungsten

w(s) w(g)

W03(s)

• 1270.2

149.6

• 1789

t73.8 55.0 130.9 164.6

• 557.3
• 39
• 781.1

114.9

• 1

140.1 97 .l

• 561.9

54.4

• 1340.9

117.0 0.096 236.7 79.7 49.7 83.7

• 1 l 1 6 . 5

t2.4

• 33.4
• 27.7

J L . I

32.6 167.8 228.2 430.9 22 29t.5 62.0 205.8 122

• 300.1

248.2

• 37

r.1 256.8

• 744.6

18.5

• 754.4

129.5 *690.0 156.9

• 744.6

18.5

• 522.5

67 51.2 0.1 44.r 266.2 168.5

• 440.1

258.6

• 432.2

365.8

• 251.9

57.2

• 51

5.8 49.0 428.4

• 737.2
• 726.3
• 888.8

807.1

30.7 180.3 252.3 353.2 50.6

J L . O

t7 4.0

AHi (kJlmol) AGi (kJlmol) S" (J/mol 'K)

• 557.7
• 333.8
• 328.9

118.4 377.8

227.r

29.7 450.0

• 687.0
• 1 6 1 5 . 0

34.3

• 9r0.7

80.3 284.9 105.79

• 100.4
• r27.0
• 204.6
• 6 1 . 8
• t ) 4 4
• 3 l . l
• 32.6
• 715.9

t07.5

• 240.34
• 3 6 1 . 1
• 4tr.2
• 407.2
• 365.8
• 576.6
• 950.8
• 1125.5
• 287.8
• 467.9
• 447.5
• 425.8
• 470.r
• 260.2
• t t J U./
• 4t4.2
• 510.9

336.0 187.0 r5.9 405.5

• 619.8
• 1572.8

56.9

• 856.3

127.3 246.0 77.11

• 96.9
• r09.8
• 185
• 66.2

_ 1? ,1

• n.2
• 40.7
• 618.4

77.0

• 26r.9
• 349.0
• 384.

I

• 393.1
• 262.3
• 546.3
• 851.0
• 992.8
• 286.1
• 367.0
• 373.2
• 379.7
• 4r9.2
• 218.4
• 1044.4
• 375.5
• 447.7

34.6 174.8

^ a A +L..t

176.7 219.0 18.8 168.0 239.7 282.8 204.6 41.5 272.7 42.6 t73.0 73.45 107.1 96.3 84 115.5 140.9

tzr.3

144.0 200.4 5 i.3 t53.7 58.45 86.8

72.r

l 1 5 . 5 t23.4 5 1 . 1 101.7 113.0 98.5 116.5 205.4 64.4 48.2 115.9 135.0 75.1 9s.0

• 1387.1
• t9r7

164.4

• 545.51
• 828.9
• 1220.1
• 592.0
• 1453.1

0.3 277.2 t28.6 t02.3 41.8

• r22A.5
• 1 7 . 7
• 20.6
• 39.4
• 245.6
• 296.8
• 395.7
• 909.3
• 886.5
• 8

r4.0

• 909.3
• 648.5
• 2.1

301.2

• 5 1 1 . 3
• 47t.5
• 280.7
• 577.6

U 473.0

• 804.2
• / o).L
• 944.0

849.4

• 842.9
• 764.0

75.9 (continued

• n

the next page)

SLIDE 24

A-12

Substance U'anium u(s)

u(s)

UF1,(s)

uFok)

U02(s) Vanadium V(s)

v(s)

533.0

• 2197.0
• 2147.4
• r0Bs.0

514.2

48[J.4

• 2068.5
• 2063.7
• 1031.8

754.4 A P P E N D I X I I : U S E F U L I ] A T A

AHf (kJlmol) AGfl (kjlmol) S'(J/mol

. K) 50.2 199.8

J/. / .()

377.9 77.0 28.9 182.3 Substance Zinc Zn(s) Zn(g)

• ) - l - .

L n - ' \ t r t l )

ZnCl2(s) Zn0(s) ZnS(s, zinc blencie) ZnS0a(.s)

AHf (k.Jimof)

(.1

130.4

• 153..19
• -4i5.i
• 3.50.-5
• 206.0
• 982.8

AGi (kJlmol)

94.8

• 147.1

*361).4

• 320.5
• 201.3
• 871.5

,5" (J/rrol . ur |\,

41.6 1 6 1 . 0 _ i 09.8 1 1 i . 5 43.7 I 10.5

G.&qmmmx*m ffi q u-unfi $hbnils,xm ffimnnmfrffi $"$frffi Dissociation Constants for Acids at 25 "C

Name Acetic Acetylsalicylic Adipic Arsenic Arsenous Ascorbic Benzoic Boric Butanoic Carbonic Chloroacetic ChloroLrs Citric Cyanic Formic Hydraz.oic Hydrocyanic HydroflLroric Hydrogen chromate ion Hydror:en peroxicle Hydrogen selenate ion Hydrosulf uric Hydrotelluric

Formula

HC)H301 HCeH704 H,C6Hs04 H.3As0a H,;As(); H2C6H606 HC7H502 HrBOs HC4Hi0, H,COI HC,Hr0rCl HCIO, I{.iC6H507 HCNO

ttcH0r HN.' HCN H F HCrOf Hro2 HScOa- H:S H2Te Name Hypobromous Hypochlorous Hypoiodous Iodic Lactic Maleic Makrnic Nitrous 0xalic Paraperiodic Phenol Phosphoric Phosphorous Propanoic PyrLrvic: Pyrophosphoric Selenous SLrccinic SLrliuric SulfuroLrs Tartaric ]j'ichloroacetic Trifluoroacetic acid

K^..

. J

4.1 x l0-r3

l r t w r n - 7

,/

na 6.3 x l0-l 2 . 5 X l 0 - r 1 3 X l0-rt 4 X 10-4 2.5 X i0-r0

K^, Ku, l . B x l 0 - 5 3.3 X l0-" 3.9 X l()-s 3.9 X 10-6 5 . - 5 X 1 0 3 t . 7 x t 0 - / - 5 . 1 x l 0 r 0 g.0 x lO-s 1.6 x l0-rl 6.5 X I0-s 5 . 4 X 1 0 - r 0 1.5 x 10-s 4.3 x l0-7 5.6 x t0 rr 1.4 x i0-r 1 . 1 x l 0 - 2

_ 5 . 1 X l 0

• 1 1

7.4 x l()-4 1.7 x to s 4.0 x t() 7 2 x 1 0 4 l . g x l 0 - 4 2.5 X 10-s 4.9 x 10-1q 3.-5 X 10-',1 3.0 x l0-7 2.4 X rc-12 2.2 X rc-) 8 . 9 x l o - 8 l x l o - l ' ) 2.3 x t0-3 t.6 X l0 rl Formula Ku, K^, HBr0 2.8 X l0 ') HCIO 2.9 x lo-8 HIO 2.3 X 10 rr HIOr 1.7 X 10 I IlcrHs()r 1.4 .Y. l0 'r H]C4H.,O4 1.2 X I0-r 5.9 X l0 7 H)C.r[],o{ 1,-5

• Y. l0-r 2.0

x l0-n HN0r 4.6 X t0 '.r HzC'01 5.9 X 10- r 0.4 X 10- 5 Hsl0(, 2.g x lo i _5.-t x l0-') HC(,I-ls() 1.3 X t0 r0 HrPOi 7.-5 X 10 j 6.2 X l0-N H r P O r 5 x l 0 r 2 . 0 x 1 0 - 7 H(.ri{qt). l..r \ l(} : l-lcrH.r0 r 4.1 x 10- t H4P'07 1.2 x l0 ' 7.9 I 10-t H,Se01 2.4 X l()-i 4.g x l0-') HrC4H401 6.1 x t0-5 2.3 x l0 (' l-1,S01 Stroncacid 1.2 X l0 2 H,SOr 1.7 x l0 r 6.4 x l0 3 H,C4I'1406 1.0 X l0-t zl.6 X l0 s HC,ChOr 2.2 x l0 | l{c,F.r0, 3.0 x l0- I

K^^

* J

• 2. Dissociation

Constants fon Hydrated Metal lons at p5 'C

iation

• t +

FL'. n r : l *

l \ |

• ., )+

PLr-

5n-

• ) +

Lt1-

Cation

,r t.l-f nl

Be2+

,. r+ t,o- ^ l +

I l " -

^ l +

L u -

• ) +

fe-

Hydrated lon Al(Hro)63+ Be(It20),,1+ Co(H20)n2+ Cr(H,,0)r;r+ Cu(H,0)6} Fe(H'0)62+

K ,\a

_ - q

1 . 4 x l 0 ' 3 X i0-7 r.3 x 10-:' 1 . 6 x 1 0 " 3 X l0-n

_ t l

3 . 2 { 1 0 ' "

Hydrated lon

Fe(H,0)6ll Ni(FI,(-))62+ Pb(Hro)(,r I Sn(H,0)62r Zn(H,0),.1+

SLIDE 25

w

".,i- ",;' ':

• .-'

.; ' '.i.

I : - - t : ' t l , ' - : r - l * : :

;i- .rj- ,* ]1**" 1--' 1o* "i,- ,',,.,.,-.,i*

A. Atomic Golors

Atomic number: Atomic symbol: Atomic number: Atomic symbol: Atomic number: Atomic symbol:

B. Standard Thermodynamic Guantities for Selected Substances at e5 "C

4

W

Be

1 2

@

Mg 29

@

rw

v

Cu 1

#

H 1 l

ffim

ffi

v Na

20

ffi

Ca 1 9

W

K

8

IUtsTL E E w

• @

CI

7

ffi

N

6 ^-. E

r

• C

1 5

m mrmn w Ev

P 5

ffi

W

B 30

@

Zn

AHi (kJlmol) AGi (kJlmol) S'(J/mol . K)

35

• L

E

xsm

E E wUZ

Br 53

@

w w

• I

Substance

Aluminum Al(s)

Al(s)

rt13+(aq) AlC13(s) A1203(s) Barium Ba(s) Ba(g) Ba?+(aq) BaC03(s) BaCl2(s) Ba0(s) Ba(0H)2(s)

330.0

• 538.4
• 704.2
• t675.7

i80.0

• 537.6
• t213.0
• 855.0
• s48.0
• 944.7

289.4

• 483
• 628.8
• 1582.3

146.0

• 560.8
• n34.4
• 806.7
• 520.3

28.32 t64.6

• 325

109.3 50.9 62.5 t70.2 9.6 r12.l 123.7 72.1

Substance BaS0a(s) Beryllium Be(s) Be0(s) Be(0H)u (s) Bismuth Bi(s) BiCl3(s) Bi203(s) Bi2S3(s) Boron B(s)

B(s)

AHi ftJ/mol)

• t473.2
• 609.4
• 902.5
• 379.1
• 573.9
• i43.

i 565.0 AGf (kJ/mol) S" (j/mol .K)

• t362.2

132.2 9.5

• 580.1

13.8

• 815.0

45.5 56.7

• 315.0

177.0

• 493.7

151.-5

• 140.6

200.4 5.9 521.0 153.4 (continued

• n

the next page)

I 6

A-7

SLIDE 26

A.B

A P P E N D I X I I : U S E F U L DATA

AGi (kJlmot)

• 388.7
• 1119.4

87.{',

• 1194.3
• 968.9

82.4 3.1

• 102.8
• 53.4

77.3

• 77.6
• 343.9
• 228.7
• 156.5
• 822.7

144.0

• 553.6
• 64.9
• 1129.1
• 748.8
• 117-5.tr
• t42.s
• 742.8
• 603.3
• 897.5
• 1322.0
• 3884.7

2.9 671.3

• -50.5
• 60.2
• o).t
• 73.7
• 62.3
• 66.4
• 102.5
• 361.4

32.7 * 166.6

• 162.3

209.9 68.4

Substance BCl3fu)

BF:(g) BzHok) 8203(s) H3803(s) Bromine Br(g) Br2(/)

Brzk)

Br-(aq) HBr(g) Cadmium Cd(s) cd(g) cdz+(aq) CdClz(s) Cd0(s) CdS(s) CdS0+(s) Calcium Ca(s) ca(g) ^ )+, La- \aq) CaC2(s) CaC03(s) CaCl2(s) CaF2(s) CaH2(s) Ca(N03)2(s) Ca0(s) Ca(0H):(s) CaS0a(s) Ca3(P0a)2(s) Carbon C(s, graphite) C(s, diamond)

c(g) cH+(g)

CH3CI(g) cH2cl2Q) cH2cl2(/) . cHCl3(/) CCI+(g) ccl4(/) CH20(g) CH202(1, fonnic acid) CH3NH2(g, methylamine) cH30H(/) CH30H(g) CzHzk) czH+(g)

AHi (kJ/mol)

• 403.8
• i

136.0

1 / I

JO.+

• t273.5
• 1094.3

I 1 1 . 9 30.9

• 1 ) 1 4
• 36.3

1 1 1 . 8

• 75.9
• 391.5
• 258.4
• 161.9
• 933.3

177.8

• 542.8
• 59.8
• t207.6
• 7q\ 4
• 1228.0
• 1 8 1 . 5
• 938.2
• 634.9
• 985.2
• 1434.5
• 4120.8

I.BB 716.7

• 7 4.6
• 8 r . 9
• 95.4
• 1 ' l A 1

L L A . L

• 134.1
• 95.7
• 128.2
• 108.6
• 425.0
• 22.5
• 238.6
• 201.0

))'7 4

52.4

S'(J/mot.K)

?q0 I

254.4 232.1 54.0 90.0 ' 175.0 r52.2 245.5 80.71 198.7 51.8 167.7

• 73.2

I 1 5 . 3 54.8 64.9 123.0

+ I . O

t54.9 *53.1 70.0 9r.7 108.4 68.5 41.4 193.2 38. l 83.4 106.5 236.0 5.7

) 4

158.1 r 86.3 234.6 270.2 177.8 201.7 309.7 216.4 218.8 129.0 242.9 126.8 239.9 200.9 219.3

Substance CzHok) c2H-50H(/)

C2H5OH(g)

C2H3Cl(g vinyl chloride) C zH 4clz(1, di chl

• ro

e th an e ) C2Ha0(g acetaldehyde) C1H4OzQ, acetic acid) C:Hsk) CaH60(/, acetone) C3H70H(i, isopropanol ) c+Hro(/) CaHrok) coHe(/) C6H5NH2(/, aniline) C6H50H(s, phenol) C6H1206(s, glucose) csHr8(/) C16Hs(s, naphthalene) C12H22011(s, sucrose)

AHi (kJ/mot) AGi (kJi mot) S" (Umot.K) co(g) cozk)

co2@q)

co?-tuq)

HCol(aq) H2cQ@q) CN-(a4) HCN(/) HCN(g)

csz(/) CSzk) c0cr2fu)

C,;o(s)

C"rium

Cs(s) cs(g)

^ + , Ls \aq) CsBr(s) CsCI(s) CsF(s) Csl(s) Chlorine cl(g)

clzk) Ct-(aq)

HCI(g) HCt(aq) clo2Q) Cl2o(g) Chromium Cr(s)

c(g)

Cr3+(aq)

• 84.68
• 277.6
• 234.8

) / . L

• 166.8
• 166.2
• 484.3
• 103.85
• 248.4
• 318.

r

• 1 4 7 7
• r25.7

49.1 3t.6

• 165.r
• 1273.3
• 250.I

78.5

• 2226.1
• 1r0.5
• 393.5
• 413.8
• 677

.r

• 692.0
• 699.7

1 5 1 108.9 i35. r 89.0 116.7

• 219.r

2327.0 76.5

• 258.0
• 400
• 438
• 553.5
• 32.0
• 174.8
• 167

.9 53.6

• 79.6
• 133.0
• 389.9
• 155.6
• 15.0
• 15.71

124.5 149.2

• 50.4
• 910.4

201.6

• 1544.3
• r37.2
• 394.4
• 386.0
• 527.8
• 586.8
• 623.2

r66 125.0

t ) 4 7

64.6 67.1

• 204.9

2302.0 49.6

• 292.0
• 387
• 414
• 525.5
• 337

105.3

• t3t.2
• 95.3
• r3t.2

120.5

97.9 351.8

229.2 160.7 281.6 264.0 208.5 263.8 159.8 270.3 199.8 1 8 1 . 1 231.0 310.0 173.4 191.9 144.0

1 1 1 1 a t L . l

t67.4 360.24 197.7

z 1 ) . 6 1 t / . 6

• s6.9

9r.2

t87.4 1 1 8 112.8 201.8 1 5 1 . 3 237.8 283.5 426.0 85.2 175.6 t32.1 t17 101.2 92.8

r27

165.2

223.r

)o.o 186.9 50.)

/50.d, too.L

23.8 t74.5

I / . t . J

• t67

.l

• 92.3
• 167

.2 t02.5 80.3 396.6

• r971

SLIDE 27

A P P E N D I X I I : U S E F U L D A T A

A-9

Substance

cro]-tuq)

C1203(s)

Cr2ol-fuq)

Cobalt Co(s) co(g) Co0(s) Co(0H)z(s) Copper Cu(s) cu(g)

^ + l

LU \aq) ^ )+/ Lv- taq) CuCl(s) CuCl2(s) CuO(s) CuS(s) CuS0q(s) Cu20(s) Cu2S(s) Fluorine F(g) Fzk) F-(aq) HF(g) Gold Au(s) Au(g) Helium He(g) Ilydrogen H(g)

u*(aq)

H-(g)

ulki

Iodine I(g) Iz(s)

Izk) r-(aq)

HI(g) Iron Fe(s) Fe(g) Fez+ (aq) Fer+(aq) FeC03(s) FeCl2(s) FeClj(s) AHi (kJlmol)

• 872.2
• 1139.7
• 1476

424.7

• 237.9
• 539.7

337.4 5 1 . 9 64.9

• r37.2
• 220.1
• t57

.3

• 53.1
• 7 7 1 4
• 168.6
• 79.5

79.38

• 335.35
• 273.3

366. l 2 iB.0 1536.3 106.76 62.42

• 56.78

26.5 4t6.3

• 87.9
• 47.69
• 740.6
• 341.8
• 399.5

AGi (kJlmol)

• 717.r
• 1058.1
• 1279

380.3

1 r / a

• L r+.^/.
• 454.3

297.7 50.2 65.5

• I19.9
• 175.7
• t29.7
• 53.6
• 662.2
• 146.0
• 86.2

/ ^ a

OL.J

• 278.8
• ) 7 \ 4

326.3 203.3 l5 17, I 70.2 19.3

• 5t.57

r.7

370.7

• 84.94
• 10.54
• 666.7
• 302.3
• 334.0

S" (J/mol .K)

44 81.2 238 30.0 179.5 53.0 79.0 33.2 166.4

• 26
• 98

86.2 108. I 42.6 66.5 r09.2 93.1 r20.9 158.75 202.79

• 13.8

173.8 47.4 180.5 t26.2 t14.7 108.9 t30.7 r80.79 I 16.14 260.69 106.45 206.6

L / . )

180.5 113.4 293.3 92.9 1 1 8 . 0 142.3 Substance Fe0(s) Fe(0H):(s) FeS2(s) Fe203(s) Fe30a(s) Lead Pb(s) Pb(g) vbz+(aq) PbB12(s) PbC0:(s) PbCl2(s) Pbl2(s) Pb(N0:)z(s) Pb0(s) PbOz(s) PbS(s) PbS0a(s) Lithium Li(s) Li(g) Lt+(aq) LiBr(s) LiCl(s) LiF(s) Lil(s) LiNO3(s) Li0H(s) Li20(s) Magnesium Mg(s) Mg(g) tttg2+ (a4) MSCI2(s) MgC03(s) VIgF2(s) MgO(s) Mg(0H)2(s) MgS0a(s) lvl93N2(s) Manganese Mn(s) Mn(g) Mn2+(aq) NIn0(s) Mn02(s) Mn0f(aq) Mercury

Hs(/) Hsk)

AHi (kJlmol)

• 272.0
• 823.0
• t78.2
• 824.2
• 1 1 1 8 , 4

r95.2 0.92

• 278.7
• 699.r
• 359.4
• 175.5
• 45

r.9

• 2t7.3
• 277.4
• 100.4
• 920.0

159,3

• 278.47
• 351.2
• 408.6
• 616.0
• 270.4
• 483.

r

• 487.5
• 597.9

147.1

• 467.0
• 64t.3
• 1095.8
• 1124.2
• 601.6
• 924.5
• t284.9
• 461

280.7

• 2r9.4
• 385.2
• 520.0
• 529.9

6 1 . 4 AGf (kJlmol) S'(J/mol . K)

• 255.2

64.75

• 696.5

106.7

• 166.9

52.9

• 742.2

87.4

• 1015.4

t46.4 162.2

• 24.4
• 26t.9
• 625.5
• 3 1 4 . 1
• r73.6

64.8 175.4 18.5 161.5 1 3 1 . 0 136.0 t74.9 * r87 .9 68.7

• 2173

68.6

• 98.7

9r.2

• 813.0

148.5 29.r 126.6 138.8

• 293.3

t2.24

• 342.0

74.3

• 384.4

5.9.3

• 587.7

35.7

• 270.3

86.8

• 381.1

90.0

• 4415

42.8

• 561.2

37 .6 32.7 rr2.5 148.6

• 455.4
• 137
• 591.8

89.6

• 1012.1

65.7

• 1071.1

57 .2

• 569.3

27.0

• 833.5

63.2

• 1170.6

9r.6

• 401

88 32.0 238.5 173.7

• 22s.6
• 78.8
• 362.9

59.7

• 465.1

53.1

• 436.2

190.6 75.9 31.8 175.0 (continuetl

• n

the next page)

SLIDE 28

A-10

Substance tlg2+(aq)

) + ,

n9z- \a4) HgCl2(s) HgO(s) HgS(s) H92Cl2(s) Nickel Ni(s) Ni(g) NiCl2(s) Ni0(s) NiS(s) Nitrogen N(g) Nz(g) NF:(g) NHik) NH3(c4) Nun+(aq) NHaBr(s) NHaCI(s) NHaCN(s) NHaF(s) NHaHC0j(s) NHal(s) NHaNO3(s) NHaN03(a4) HN0rk) HN03(a4) No(g)

Nozk)

N03 (aq)

N0Br(g) N0cl(g) NzH+(/) NzHak) Nzo(g) Nzo+(/) Nzo+(g)

N205(s)

Nzosk) Orygen

• (s)
• z(g)
• :(g)

OH-(aq) Hzo(/) Hzo(g) H202(/) H:ozk)

AHi (kJlmol)

170.21 166.87

a a / a

• /z+.J
• 90.8
• 58.2
• 265.4

429.7

• 305.3
• 239.7
• 82.0

472.7

• 1 3 2 . 1
• 45.9
• 80.29
• 133.26
• 270.8
• 314.4

0.4

• 464.0
• 849.4
• 201.4
• 365.6
• 339.9
• 133.9
• 207

9r.3

33.2

• 206.8s

82.2 51.7 s0.6 95.4 8 1 . 6

• 19.5

I l . t

• 43.1

I J.J

249.2 142.7

• 230.02
• 285.8
• 24r.8
• 187.8
• 136.3

AGf (kJlmol)

164.4 153.5

• 178.6
• 58.5
• 50.6
• 2r0.7

384.5

• 259.0
• 2 n . 7
• 79.5

455.5

• 90.6
• t6.4
• 26.50
• 79.3r
• 175.2
• 202.9
• 348.7
• 665.9
• 112.5
• 183.9
• 190.6
• 73.5
• 110.9

87.6 5 1.3

• i 10.2

, 82.4 66. I r49.3 t59.4

r03.7

97.5 99.8 113.9 n7.I 231.7 163.2

• 157

.3

• 237.r
• 228.6
• 120.4
• 105.6

S" (J/mol .K)

• 36.19

65.74 146.0 70.3 82.4 191.6 29.9

r82.2

97.7 37.99 53.0 153.3 1 9 1 . 6 260.8 192.8 i 1 1 . 3 r1t.I7 113.0 g/,.6 72.0

1 l n

• I

17.0 l5 1.1 259.8 266.9 r46 210.8 240.1 t46.70 273.7 26r.7

r2r.2

238.5 220.0 209.2 304.4 178.2 355.7 l 6 t . t 205.2 238.9

• 10.90

70.0 188.8. 109.6 232.7 Substance Phosphorus P(s, white) P(s, red) P(g) PzQ) P+(g) PCI3(/) PClrk) PCls(s) PCl5ft) PFsk) PHrk) P0c]3(/) P0Clj(g)

Pof-tuq) HPof-@q)

H2POa @q) H3P0a(s) \Poa@q) Pa06(s) Pa016(s) Platinum Pt(s)

Pt(s)

Potassium I((s)

K(s)

x*(aq) KBr(s) I(CN(s) KCI(s) KCl0r(s) KCi0a(s) KF(s) Ifl(s) KN03(s) K0H(s) KoH(aq) K02(s) K2C03(s) K20(s) K202(s) K2S0a(s) Rubidium Rb(s) Rb(g) Rb+(aq) RbBr(s) RbCl(s) RbClO3(s)

AHi fiJlmol)

• r7.6

316.5 r44.0 58.9

• 319.7
• 287.0
• 443.5
• 374.9
• 1594.4

5.4

• 597.1
• 558.5

1 ^ - - '

• t / / t u
• 1292.r
• t296.3
• 1284.4
• 1288.3
• 1640.1
• 2984

56s.3 89.0

L J L . L 1

• 393.8
• I13.0
• 436.5
• 397.7
• 432.8
• 567.3
• 327.9
• 494.6
• 424.6
• 482.4
• 284.9
• 1 1 5 1 . 0
• 36r.5
• 494.1
• 1437.8

80.9

• 25r.12
• 394.6
• 435.4
• 392.4

AGi (kJlmol)

• 1 2 . 1

280.1 103.5 24.4

• 272.3
• 267.8
• 305.0
• 1520.7

13.5

• 520.8
• 512.9
• 1018.7
• 1089.2
• t130.2
• t124.3
• 1142.6
• 2698

U

520.5 60.5

• 283.3
• 380.7
• 101

.9

• 408.5
• 296.3
• 303.

r

• 537.8
• 324.9
• 394.9
• 379.4
• 440.5
• 239.4
• r063.5
• 322.1
• 4) \

1

• 1321.4

53. r

• 283.1
• 381

.8

• 407.8
• 292.0

S" (j/mot.(y

4 1 . 1 22.8 163.2 2 l8.l 280.0 2r7.1 3 1 1 . 8 364.6 300.8

) 1 n )

1 a . F

325.5

• ) ? n c
• . ) ' l ' r

90.4 I10.5 158.2 228.9 41.6 192.4 64.7 160.3 101.2 95.9 128.5 82.6 143.1 r 51.0 66,6 106.3

I J J . I

8r.2

91.6 n6.7 155.5 94.14

102.r

t75.6 76.8 170.1

rzt.75

110.0 95.9 152 A P P E N D I X I I : U S E F U L D A T A

''"rt:, ,*, i'

SLIDE 29

A P P E N D I X l l : U S E F U L D A T A A - 1 1

AHiftJ/mol) AGi (kJlmol) S'(J/mol' K)

Substance RbF(s) Rbi(s) Scandium Sc(s) sc(g) Selenium Se(s, gray) se(g) H2Se(g) Silicon Si(s)

si(s)

sicl4(/) SiFa(g) siHaQ) Si02(s, quartz) si2H6Q) Silver Ag(s)

Ag(s)

. + ,

Lg'\aq) AgBr(s) AgCl(s) AgF(s) Agl(s) AgNO3(s) Ag20(s) Ag2S(s) Ag2S0a(s) Sodium Na(s) Na(g) Na-(a4) NaBr(s)

Ndct(s)

NaCl(ar1) NaCl03(s) NaF(s) NaHC0:(s) NaHS0a(s) Nal(s) NaN0:(s) NaN03(aq) NaOH(s) NaOH(aq) NaO2(s) Na2C03(s) Na20(s) Na202(s)

Substance

Na2S0a(s) Na3P0a(s) Strontium Sr(s) Sr(g)

s4+@q)

SrCl2(s)

srior(s) Sr0(s)

SrS0a(s) Sulfur S(s, rhombic) S(s, monoclinic)

s(g) szk)

Ssk) s2-(oq) sFok) HS-(aq) Hzs(g) H2S(aq) socl2(/)

sozk) sor(g) s0f-(aq) HS0f(a4)

H2So4(/) H2SO4@q)

svol-bq)

Tin Sn(s, white) Sn(s, gray) sn(g) SnCl+(/) SnCI+(g) Sn0(s) Sn02(s) Titanium Ti(s)

ri(g) ric14(i) ricLk)

Ti02(s) Tungsten

w(s) w(g)

W03(s)

• 1270.2

149.6

• 1789

t73.8 55.0 130.9 164.6

• 557.3
• 39
• 781.1

114.9

• 1

140.1 97 .l

• 561.9

54.4

• 1340.9

117.0 0.096 236.7 79.7 49.7 83.7

• 1 l 1 6 . 5

t2.4

• 33.4
• 27.7

J L . I

32.6 167.8 228.2 430.9 22 29t.5 62.0 205.8 122

• 300.1

248.2

• 37

r.1 256.8

• 744.6

18.5

• 754.4

129.5 *690.0 156.9

• 744.6

18.5

• 522.5

67 51.2 0.1 44.r 266.2 168.5

• 440.1

258.6

• 432.2

365.8

• 251.9

57.2

• 51

5.8 49.0 428.4

• 737.2
• 726.3
• 888.8

807.1

30.7 180.3 252.3 353.2 50.6

J L . O

t7 4.0

AHi (kJlmol) AGi (kJlmol) S" (J/mol 'K)

• 557.7
• 333.8
• 328.9

118.4 377.8

227.r

29.7 450.0

• 687.0
• 1 6 1 5 . 0

34.3

• 9r0.7

80.3 284.9 105.79

• 100.4
• r27.0
• 204.6
• 6 1 . 8
• t ) 4 4
• 3 l . l
• 32.6
• 715.9

t07.5

• 240.34
• 3 6 1 . 1
• 4tr.2
• 407.2
• 365.8
• 576.6
• 950.8
• 1125.5
• 287.8
• 467.9
• 447.5
• 425.8
• 470.r
• 260.2
• t t J U./
• 4t4.2
• 510.9

336.0 187.0 r5.9 405.5

• 619.8
• 1572.8

56.9

• 856.3

127.3 246.0 77.11

• 96.9
• r09.8
• 185
• 66.2

_ 1? ,1

• n.2
• 40.7
• 618.4

77.0

• 26r.9
• 349.0
• 384.

I

• 393.1
• 262.3
• 546.3
• 851.0
• 992.8
• 286.1
• 367.0
• 373.2
• 379.7
• 4r9.2
• 218.4
• 1044.4
• 375.5
• 447.7

34.6 174.8

^ a A +L..t

176.7 219.0 18.8 168.0 239.7 282.8 204.6 41.5 272.7 42.6 t73.0 73.45 107.1 96.3 84 115.5 140.9

tzr.3

144.0 200.4 5 i.3 t53.7 58.45 86.8

72.r

l 1 5 . 5 t23.4 5 1 . 1 101.7 113.0 98.5 116.5 205.4 64.4 48.2 115.9 135.0 75.1 9s.0

• 1387.1
• t9r7

164.4

• 545.51
• 828.9
• 1220.1
• 592.0
• 1453.1

0.3 277.2 t28.6 t02.3 41.8

• r22A.5
• 1 7 . 7
• 20.6
• 39.4
• 245.6
• 296.8
• 395.7
• 909.3
• 886.5
• 8

r4.0

• 909.3
• 648.5
• 2.1

301.2

• 5 1 1 . 3
• 47t.5
• 280.7
• 577.6

U 473.0

• 804.2
• / o).L
• 944.0

849.4

• 842.9
• 764.0

75.9 (continued

• n

the next page)

SLIDE 30

A-12

Substance U'anium u(s)

u(s)

UF1,(s)

uFok)

U02(s) Vanadium V(s)

v(s)

533.0

• 2197.0
• 2147.4
• r0Bs.0

514.2

48[J.4

• 2068.5
• 2063.7
• 1031.8

754.4 A P P E N D I X I I : U S E F U L I ] A T A

AHf (kJlmol) AGfl (kjlmol) S'(J/mol

. K) 50.2 199.8

J/. / .()

377.9 77.0 28.9 182.3 Substance Zinc Zn(s) Zn(g)

• ) - l - .

L n - ' \ t r t l )

ZnCl2(s) Zn0(s) ZnS(s, zinc blencie) ZnS0a(.s)

AHf (k.Jimof)

(.1

130.4

• 153..19
• -4i5.i
• 3.50.-5
• 206.0
• 982.8

AGi (kJlmol)

94.8

• 147.1

*361).4

• 320.5
• 201.3
• 871.5

,5" (J/rrol . ur |\,

41.6 1 6 1 . 0 _ i 09.8 1 1 i . 5 43.7 I 10.5

G.&qmmmx*m ffi q u-unfi $hbnils,xm ffimnnmfrffi $"$frffi Dissociation Constants for Acids at 25 "C

Name Acetic Acetylsalicylic Adipic Arsenic Arsenous Ascorbic Benzoic Boric Butanoic Carbonic Chloroacetic ChloroLrs Citric Cyanic Formic Hydraz.oic Hydrocyanic HydroflLroric Hydrogen chromate ion Hydror:en peroxicle Hydrogen selenate ion Hydrosulf uric Hydrotelluric

Formula

HC)H301 HCeH704 H,C6Hs04 H.3As0a H,;As(); H2C6H606 HC7H502 HrBOs HC4Hi0, H,COI HC,Hr0rCl HCIO, I{.iC6H507 HCNO

ttcH0r HN.' HCN H F HCrOf Hro2 HScOa- H:S H2Te Name Hypobromous Hypochlorous Hypoiodous Iodic Lactic Maleic Makrnic Nitrous 0xalic Paraperiodic Phenol Phosphoric Phosphorous Propanoic PyrLrvic: Pyrophosphoric Selenous SLrccinic SLrliuric SulfuroLrs Tartaric ]j'ichloroacetic Trifluoroacetic acid

K^..

. J

4.1 x l0-r3

l r t w r n - 7

,/

na 6.3 x l0-l 2 . 5 X l 0 - r 1 3 X l0-rt 4 X 10-4 2.5 X i0-r0

K^, Ku, l . B x l 0 - 5 3.3 X l0-" 3.9 X l()-s 3.9 X 10-6 5 . - 5 X 1 0 3 t . 7 x t 0 - / - 5 . 1 x l 0 r 0 g.0 x lO-s 1.6 x l0-rl 6.5 X I0-s 5 . 4 X 1 0 - r 0 1.5 x 10-s 4.3 x l0-7 5.6 x t0 rr 1.4 x i0-r 1 . 1 x l 0 - 2

_ 5 . 1 X l 0

• 1 1

7.4 x l()-4 1.7 x to s 4.0 x t() 7 2 x 1 0 4 l . g x l 0 - 4 2.5 X 10-s 4.9 x 10-1q 3.-5 X 10-',1 3.0 x l0-7 2.4 X rc-12 2.2 X rc-) 8 . 9 x l o - 8 l x l o - l ' ) 2.3 x t0-3 t.6 X l0 rl Formula Ku, K^, HBr0 2.8 X l0 ') HCIO 2.9 x lo-8 HIO 2.3 X 10 rr HIOr 1.7 X 10 I IlcrHs()r 1.4 .Y. l0 'r H]C4H.,O4 1.2 X I0-r 5.9 X l0 7 H)C.r[],o{ 1,-5

• Y. l0-r 2.0

x l0-n HN0r 4.6 X t0 '.r HzC'01 5.9 X 10- r 0.4 X 10- 5 Hsl0(, 2.g x lo i _5.-t x l0-') HC(,I-ls() 1.3 X t0 r0 HrPOi 7.-5 X 10 j 6.2 X l0-N H r P O r 5 x l 0 r 2 . 0 x 1 0 - 7 H(.ri{qt). l..r \ l(} : l-lcrH.r0 r 4.1 x 10- t H4P'07 1.2 x l0 ' 7.9 I 10-t H,Se01 2.4 X l()-i 4.g x l0-') HrC4H401 6.1 x t0-5 2.3 x l0 (' l-1,S01 Stroncacid 1.2 X l0 2 H,SOr 1.7 x l0 r 6.4 x l0 3 H,C4I'1406 1.0 X l0-t zl.6 X l0 s HC,ChOr 2.2 x l0 | l{c,F.r0, 3.0 x l0- I

K^^

* J

• 2. Dissociation

Constants fon Hydrated Metal lons at p5 'C

iation

• t +

FL'. n r : l *

l \ |

• ., )+

PLr-

5n-

• ) +

Lt1-

Cation

,r t.l-f nl

Be2+

,. r+ t,o- ^ l +

I l " -

^ l +

L u -

• ) +

fe-

Hydrated lon Al(Hro)63+ Be(It20),,1+ Co(H20)n2+ Cr(H,,0)r;r+ Cu(H,0)6} Fe(H'0)62+

K ,\a

_ - q

1 . 4 x l 0 ' 3 X i0-7 r.3 x 10-:' 1 . 6 x 1 0 " 3 X l0-n

_ t l

3 . 2 { 1 0 ' "

Hydrated lon

Fe(H,0)6ll Ni(FI,(-))62+ Pb(Hro)(,r I Sn(H,0)62r Zn(H,0),.1+