chemistry 161 revision chapters 4-6 chem.hawaii/bil301/welcome.html
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CHEMISTRY 161 Revision Chapters 4-6 www.chem.hawaii.edu/Bil301/welcome.html. 4. CHEMICAL REACTIONS. 4.1. properties of solutions 4.2. reactions in solutions a) precipitation reactions b) acid-base reactions (proton transfer) c) redox reactions (electron transfer). - PowerPoint PPT PresentationTRANSCRIPT
CHEMISTRY 161
Revision Chapters 4-6
www.chem.hawaii.edu/Bil301/welcome.html
4. CHEMICAL REACTIONS
4.1. properties of solutions
4.2. reactions in solutions
a) precipitation reactions
b) acid-base reactions (proton transfer)
c) redox reactions (electron transfer)
non-electrolyte weak electrolyte strong electrolyte
methanol
sugar
ethanol
water
dark bright
ionic compounds
NaOH
HCl
H2SO4
CH3COOH
HCOOH
HF
medium
DISSOCIATION
‘breaking apart’
NaCl (s) → Na+ (aq) + Cl- (aq)
NaOH (s) → Na+ (aq) + OH- (aq)
HCl (g) → H+ (aq) + Cl- (aq)
strong electrolytes are fully dissociated
weak electrolyte
CH3COOH(aq) + H2O(l) H3O+(aq) + CH3COO-(aq)
NH3(aq) + H2O(l) NH4+ + OH-
strong electrolyte
HCl(aq) + H2O(l) → H3O+(aq) + Cl-(aq)
HNO3(aq) + H2O(l) → H3O+(aq) + NO3-(aq)
monoprotic acids
4.2.1. insoluble compounds
1.M+ compounds (M = H, Li, Na, K, Rb, Cs, NH4)
2. A- compounds (A = NO3, HCO3, ClO3, Cl, Br, I)(AgX, PbX2)
3. SO42-
(Ag, Ca, Sr, Ba, Hg, Pb)
4. CO32-, PO4
3-, CrO42-, S2-
(exception: M+)
4.2.2. ACID-BASE REACTION
acid + base → salt + water
(neutralization reaction)
HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
molecular equation – ionic equation – spectator ions
4.2.3. OXIDATION NUMBER
ionic compounds ↔ molecular compounds
NaCl HF, H2
Na+Cl- ?electrons are fully transferred covalent bond
‘oxidation number’
charges an atom would have if electrons are transferred completely
TYPES OF REDOX REACTIONS
1.combination reactions
A + B → C
2. decomposition reactions
C → A + B
3. displacement reactions
A + BC → AC + B
4. disproportionation reactions
[p] = Nm-2 = kg m-1 s-2 = Pa
SI units
5. GASES
p × V = n × R × T
1. ideal gas equation
R = 8.314 J / mol / K
Vm = 22.4 l
2. molar volume
3. Kinetic Molecular Theory of Gases
4. Distribution of Molecular Speeds
Ekin = ½ M u2 = 3/2 R T
5. Real Gas Law
(p + (a n2 / V2) ) (V – n b) = n R T
Enthalpy of Reaction
heat released or absorbed by the system at a constant pressure
H = HH = Hproductsproducts - H - HreactantsreactantsH = HH = Hproductsproducts - H - Hreactantsreactants
Hfinal > Hinitial : H > 0 ENDOTHERMICHfinal > Hinitial : H > 0 ENDOTHERMIC
Hfinal < Hinitial : H < 0 EXOTHERMICHfinal < Hinitial : H < 0 EXOTHERMIC
6. THERMOCHEMISTRY
measurement of heat changes
HHmm = = ΔΔQQmm = = ccmpmp ΔΔTT HHmm = = ΔΔQQmm = = ccmpmp ΔΔTT
ccmpmp(H(H22O) = 75.3 J molO) = 75.3 J mol-1-1 K K-1-1ccmpmp(H(H22O) = 75.3 J molO) = 75.3 J mol-1-1 K K-1-1
H = H = ΔΔQ = (Q = (ccmpmp × n + c × n + ccupcup) ) ΔΔTT H = H = ΔΔQ = (Q = (ccmpmp × n + c × n + ccupcup) ) ΔΔTT
Standard Enthalpy of Formation
HHffOOHHff
OO
heat change when 1 mole of a compound is formed from its elements at a pressure of 1 atm
(T = 298 K)
HHffO O (element) = 0 kJ/mol(element) = 0 kJ/molHHff
O O (element) = 0 kJ/mol(element) = 0 kJ/mol
HHffO O (graphite) = 0 kJ/mol(graphite) = 0 kJ/molHHff
O O (graphite) = 0 kJ/mol(graphite) = 0 kJ/mol HHffO O (diamond) = 1.9 kJ/mol(diamond) = 1.9 kJ/molHHff
O O (diamond) = 1.9 kJ/mol(diamond) = 1.9 kJ/mol
EN
TH
AL
PY
, H
HHreactantsreactantsHHreactantsreactants
HHproductsproductsHHproductsproducts
C(s, graphite) + O2(g)
CO2(g)
Hf0 = - 393.51 kJ mol-1
0
-393.51
C(s, graphite) + O2(g) CO2(g) Hf0 = - 393.51 kJ mol-1
Standard Enthalpy of Formation
C(s, graphite) + 2H2(g) CH4(g) Hf0 = - 74.81 kJ mol-1
½ N2(g) + 3/2 H2(g) NH3(g) Hf0 = - 46.11 kJ mol-1
(1/2) N2(g) + (1/2) O2(g) NO(g) Hf0 = + 33.18 kJ mol-1
HHOOrxn rxn = = ΣΣnnΔΔHHff
00(prod) – (prod) – ΣΣmmΔΔHHff00(react)(react) HHOO
rxn rxn = = ΣΣnnΔΔHHff00(prod) – (prod) – ΣΣmmΔΔHHff
00(react)(react)
Standard Enthalpy of Reaction
CaO(s) + CO2(g) → CaCO3(s)
-635.6 -393.5 -1206.9 [kJ/mol]
HHOOrxn rxn = -177.8 kJ/mol= -177.8 kJ/molHHOO
rxn rxn = -177.8 kJ/mol= -177.8 kJ/mol
1 atm = 760 mm Hg = 760 torr = 103,325 Pa
R = 8.314 J / mol / K
cmp(H2O) = 75.3 J / mol / K
p V = n R T
HHOOrxn rxn = = ΣΣnnΔΔHHff
00(prod) – (prod) – ΣΣmmΔΔHHff00(react)(react) HHOO
rxn rxn = = ΣΣnnΔΔHHff00(prod) – (prod) – ΣΣmmΔΔHHff
00(react)(react)
Ekin = ½ M u2 = 3/2 R T
ΔΔQ = (Q = (ccmpmp × n + c × n + ccupcup) ) ΔΔTT ΔΔQ = (Q = (ccmpmp × n + c × n + ccupcup) ) ΔΔTT
Come in Time!Do not forget your calculator!