Idea Transcript
Advanced Placement
Chemistry Enthalpy, Entropy and Free Energy
2014
29 Cu 63.55
30 Zn 65.39
41 Nb 92.91
42 Mo 93.94
43 Tc (98)
†Actinide Series:
*Lanthanide Series:
105 Db (262)
106 Sg (263)
107 Bh (262)
33 As 74.92
34 Se 78.96
35 Br 79.90
109 Mt (266)
110 § (269)
111 § (272)
112 § (277)
§Not yet named
79 80 78 77 84 83 82 81 Au Hg Pt Ir Po Bi Pb Tl 192.2 195.08 196.97 200.59 204.38 207.2 208.98 (209)
85 At (210)
95 Am (243)
96 Cm (247)
97 Bk (247)
98 Cf (251)
99 Es (252)
100 Fm (257)
101 Md (258)
102 No (259)
103 Lr (260)
62 63 64 65 66 67 68 69 70 71 Sm Eu Gd Tb Dy Ho Er Tm Yb Lu 150.4 151.97 157.25 158.93 162.50 164.93 167.26 168.93 173.04 174.97
108 Hs (265)
91 92 93 94 90 Th Pa U Np Pu 232.04 231.04 238.03 237.05 (244)
59 60 61 58 Ce Pr Nd Pm 140.12 140.91 144.24 (145)
88 104 89 87 † Rf Ac Ra Fr (223) 226.02 227.03 (261)
32 Ge 72.59
36 Kr 83.80
17 16 15 14 18 Cl S P Si Ar 28.09 30.974 32.06 35.453 39.948
9 10 F Ne 19.00 20.179
2 He 4.0026
86 Rn (222)
48 46 47 45 44 53 52 51 50 49 54 Cd Pd Ag Rh Ru I Te Sb Sn In Xe 101.1 102.91 106.42 107.87 112.41 114.82 118.71 121.75 127.60 126.91 131.29
56 76 75 73 74 72 57 55 * Os Re Ta W Hf La Ba Cs 132.91 137.33 138.91 178.49 180.95 183.85 186.21 190.2
40 Zr 91.22
39 Y 88.91
28 Ni 58.69
38 Sr 87.62
27 Co 58.93
37 Rb 85.47
26 25 24 Fe Mn Cr 52.00 54.938 55.85 31 Ga 69.72
23 V 50.94
21 Sc 44.96
20 Ca 40.08
19 K 39.10
22 Ti 47.90
13 Al 26.98
12 Mg 24.30
11 Na 22.99
8 7 6 5 O N C B 10.811 12.011 14.007 16.00
4 Be 9.012
3 Li 6.941
1 H 1.0079
Periodic Table of the Elements
AP Chemistry Equations & Constants ADVANCEDPLACEMENT PLACEMENTCHEMISTRY CHEMISTRYEQUATIONS EQUATIONSAND ANDCONSTANTS CONSTANTS ADVANCED Throughoutthe thetest testthe thefollowing followingsymbols symbolshave havethe thedefinitions definitionsspecified specifiedunless unlessotherwise otherwisenoted. noted. Throughout L,mL mL L, gg nm nm atm atm
== == == ==
liter(s),milliliter(s) milliliter(s) liter(s), gram(s) gram(s) nanometer(s) nanometer(s) atmosphere(s) atmosphere(s)
ATOMICSTRUCTURE STRUCTURE ATOMIC EE == hhνν λν cc == λν
mmHg Hg mm kJ J,J,kJ VV mol mol
== == == ==
millimetersof ofmercury mercury millimeters joule(s),kilojoule(s) kilojoule(s) joule(s), volt(s) volt(s) mole(s) mole(s)
energy EE == energy frequency νν == frequency wavelength λλ == wavelength −34 Planck’sconstant, constant,hh == 6.626 6.626××10 10−34 Planck’s JJss −1 mss−1 Speedof oflight, light,cc == 2.998 2.998××10 1088m Speed −1 Avogadro’snumber number == 6.022 6.022××10 102323mol mol−1 Avogadro’s −19 Electroncharge, charge,ee == −1.602 −1.602××10 10−19 coulomb Electron coulomb
EQUILIBRIUM EQUILIBRIUM [C]cc [D]dd [A] [B] [B] [A]
EquilibriumConstants Constants Equilibrium
((PPCC))cc((PPDD))dd
(molarconcentrations) concentrations) KKcc (molar (gaspressures) pressures) KKpp (gas
[C] [D] R ccCC++ddD where aaAA++bbBB R D ,,where KKcc == aa bb
KKpp ==
((PPAA))aa((PPBB))bb
[H++ ][A-- ] KKaa == [H ][A ] [HA] [HA]
KKbb ==
[OH--][HB ][HB++]] [OH [B] [B]
(weakacid) acid) KKaa (weak (weakbase) base) KKbb (weak (water) KKww (water)
−14 [H++][OH ][OH−−]] == 1.0 1.0 ××10 10−14 25°C atat25°C KKww == [H
== KKaa××KKbb pOH==−log[OH −log[OH−−]] pH == −log[H −log[H++]],, pOH pH 14 == pH pH++pOH pOH 14 [A--]] pH == pK pKaa++log log[A pH
[HA] [HA]
pKaa==−logK −logKaa,, pK pKbb ==−logK −logKbb pK KINETICS KINETICS ln[A]t t−−ln[A] ln[A]00 == −−ktkt ln[A]
11 -- 11
[[AA]]t t [[AA]]00
== ktkt
0.693 0.693 tt½ ½ == kk
rateconstant constant kk == rate time tt ==time tt½ half-life ½ == half-life
GASES, LIQUIDS, AND SOLUTIONS PV = nRT PA = Ptotal × XA, where XA =
moles A total moles
Ptotal = PA + PB + PC + . . . n= m
M
K = °C + 273 D= m V
KE per molecule = 1 mv 2 2
Molarity, M = moles of solute per liter of solution A = abc
THERMOCHEMISTRY/ ELECTROCHEMISTRY
q = mcDT = DSD Â SD products - Â SD reactants = DH D Â DHfD products - Â DH fD reactants = DGD Â DGfD products - Â DGfD reactants G D DH D - T D S D D= = - RT ln K = - n F ED I
q t
P V T n m M D KE Ã A a b c
= = = = = = = = = = = = =
pressure volume temperature number of moles mass molar mass density kinetic energy velocity absorbance molar absorptivity path length concentration
Gas constant, R = 8.314 J mol -1 K -1 = 0.08206 L atm mol -1 K -1 = 62.36 L torr mol -1 K -1 1 atm = 760 mm Hg = 760 torr STP = 0.00 D C and 1.000 atm
q m c T SD
= = = =
heat mass specific heat capacity temperature
= standard entropy D H = standard enthalpy GD = standard free energy n = number of moles E D = standard reduction potential I = current (amperes) q = charge (coulombs) t = time (seconds)
Faraday’s constant, F = 96,485 coulombs per mole of electrons 1 joule 1volt = 1 coulomb
THERMODYNAMICS Enthalpy, Entropy, Free Energy, & Equilibrium What I Absolutely Have to Know to Survive the AP Exam The following might indicate the question deals with thermochemistry and thermodynamics: calorimeter; enthalpy (ΔH); specific heat (Cp); endothermic; exothermic; heat (q); heat capacity (C); heat transfer; bond energy; entropy (ΔS); Gibb’s free energy (ΔG); spontaneous; state function
Zeroth Law: First Law: Second Law: Third Law:
Laws of Thermodynamics Heat flows from hot to cold Energy and matter are conserved Matter tends towards chaos Entropy of a pure crystal at 0K is zero
Thermodynamic Terms What does each term tell us? Enthalpy (ΔH)
Energy content
+ endothermic
− exothermic
Entropy (ΔS)
Disorder
+ increase in the dispersal of matter
− decrease in the dispersal of matter
Free energy (ΔG)
Thermodynamically favored or not favored
+ not thermodynamically favored
− thermodynamically favored
Equilibrium (K )
Extent of reaction
>1 reaction favors products
1, products favored