AP Chemistry Reference Sheet - San Leandro USD / … · AP CHEMISTRY REFERENCE SHEET EQUATIONS...
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AP CHEMISTRY REFERENCE SHEET EQUATIONS Basic Density: d = m V Kinetic energy: KE = 1 2 mv 2 Einstein’s Eq’n: E = mc 2 Atomic Structure Frequency of light: ν = c λ Energy of photon: E = h ν or E = hc λ De Broglie eq’n: λ = h mv Uncertainty Principle: Δx • mΔv ≥ h 4π Energy of Hydrogen e － levels: E n = −2.18 × 10 −18 J 1 n 2 Bonding Coulomb’s Law: E = 2.31 × 10 −19 J • nm Q 1 Q 2 r Dipole moment: μ = qr Gases, Liquids, & Solutions Ideal Gas Law: PV = nRT Van der Waal’s Eq’n: P + a n V 2 × V − nb [ ] = nRT Combined Gas Law: P 1 V 1 T 1 = P 2 V 2 T 2 Dalton’s Law: P tot = P 1 + P 2 + P 3 + ... Average Kinetic Energy: KE avg = 3 2 RT Root Mean Square Velocity: u rms = 3RT M Effusion: rate A rate B = M B M A Clausius-Clapeyron Equation: ln P vap = −ΔH vap RT + ln β ln P 2 P 1 = −ΔH vap R 1 T 2 − 1 T 1 Solution dilution: M 1 V 1 = M 2 V 2 Henry’s Law: S gas = k H P gas Raoult’s Law: P sol'n = χ solv P solv FPD: ΔT f = m × iK f BPE: ΔT b = m × iK b Osmotic pressure: Π = MRT Thermodynamics Internal energy: ΔE = q + w Heat Capacity: q = mC s ΔT Pressure-Volume Work: w = −PΔV Change in Enthalpy: ΔH = ΔE + PΔV Entropy: S = k ln W Change in Entropy of Surroundings: ΔS surr = −ΔH sys T Change in Gibb’s Free Energy: ΔG = ΔH − TΔS Free Energy (nonstandard): ΔG rxn = ΔG rxn + RT ln Q Gibb’s Free Energy and K: ΔG rxn = −RT ln K Kinetics The Rate Law: Rate = k A [ ] m B [] n Arrhenius Equation (linear): ln k = − E a R 1 T + ln A Integrated Rate Laws (0,1,2): A [ ] t = −kt + A [ ] 0 ln A [ ] t = −kt + ln A [ ] 0 1 A [ ] t = kt + 1 A [ ] 0 Equilibrium Equilibrium Constant: K eq = C [ ] c × D [ ] d A [ ] a × B [ ] b Acid Base Equilibrium: pH = − log H 3 O + [ ] pOH = − log OH − [ ] K w = H + [ ] OH − [ ] = 1.0 × 10 −14 K a = H + [ ] A − [ ] HA [ ] K b = HB + [ ] OH − [ ] B [] HendersonHasselbalch Eq’n: pH = pK a + log base acid Electrochemistry Nernst Eq’n: E cell = E cell − 0.0592 V n log Q ΔG = −nFE cell CONSTANTS 1 amu = 1.6605 × 10 － 27 kg Avogadro’s # (N A ) = 6.02214 × 10 23 mol － 1 Bohr radius (a0) = 5.2918 × 10 － 11 m Bolzmann’s const. (k) = 1.3807 × 10 -23 J/K Faraday’s const. (F) = 9.6485 × 10 4 C/mol Planck’s const. (h) = 6.6261 × 10 － 34 Js Gas const. (R) = 0.0821 (Latm)/(molK) = 8.3145 J/(molK) Electron charge (e) = 1.6022 × 10 － 19 C Mass of electron (m e ) = 9.1093826 × 10 –31 kg Mass of proton (m p ) = 1.67262171 × 10 –27 kg Mass of neutron (m n ) = 1.6749273 × 10 –27 kg Speed of light (c) = 2.9979 × 10 8 m/s
Transcript of AP Chemistry Reference Sheet - San Leandro USD / … · AP CHEMISTRY REFERENCE SHEET EQUATIONS...
AP CHEMISTRY REFERENCE SHEET
EQUATIONS Basic
Density:
€
d =mV
Kinetic energy:
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KE =12mv 2
Einstein’s Eq’n:
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E = mc 2
Atomic Structure
Frequency of light:
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ν =cλ
Energy of photon:
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E = hν or
€
E =hcλ
De Broglie eq’n:
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λ =hmv
Uncertainty Principle:
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Δx • mΔv ≥ h4π
Energy of Hydrogen e－ levels:
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En = −2.18 ×10−18 J 1n2⎛
⎝ ⎜
⎞
⎠ ⎟
Bonding
Coulomb’s Law:
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E = 2.31×10−19 J • nm Q1Q2
r⎛
⎝ ⎜
⎞
⎠ ⎟
Dipole moment:
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µ = qr
Gases, Liquids, & Solutions
Ideal Gas Law:
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PV = nRT
Van der Waal’s Eq’n:
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P + a nV⎛
⎝ ⎜
⎞
⎠ ⎟ 2⎡
⎣ ⎢
⎤
⎦ ⎥ × V − nb[ ] = nRT
Combined Gas Law:
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P1V1T1
=P2V2T2
Dalton’s Law:
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Ptot = P1 + P2 + P3 + ...
Average Kinetic Energy:
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KE avg =32RT
Root Mean Square Velocity:
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urms =3RTM
Effusion:
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rate Arate B
=MB
MA
Clausius-Clapeyron Equation:
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ln Pvap =−ΔHvap
RT+ ln β
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ln P2
P1=−ΔHvap
R1T2−
1T1
⎛
⎝ ⎜
⎞
⎠ ⎟
Solution dilution:
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M1V1 =M2V2
Henry’s Law:
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Sgas = kHPgas
Raoult’s Law:
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Psol'n = χsolvPsolv
FPD:
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ΔTf = m × iK f
BPE:
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ΔTb = m × iKb
Osmotic pressure:
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Π =MRT
Thermodynamics
Internal energy:
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ΔE = q + w
Heat Capacity:
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q = mCsΔT
Pressure-Volume Work:
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w = −PΔV
Change in Enthalpy:
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ΔH = ΔE + PΔV
Entropy:
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S = k ln W
Change in Entropy of Surroundings:
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ΔSsurr =−ΔHsys
T
Change in Gibb’s Free Energy:
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ΔG = ΔH −TΔS
Free Energy (nonstandard):
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ΔGrxn = ΔGrxn + RT ln Q
Gibb’s Free Energy and K:
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ΔGrxn = −RT ln K
Kinetics
The Rate Law:
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Rate = k A[ ]m B[ ]n Arrhenius Equation (linear):
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lnk = −Ea
R1T⎛
⎝ ⎜ ⎞
⎠ ⎟ + lnA
Integrated Rate Laws (0,1,2):
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A[ ]t = −kt + A[ ]0
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ln A[ ]t = −kt + ln A[ ]0
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1A[ ]t
= kt +1A[ ]0
Equilibrium
Equilibrium Constant:
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Keq =C[ ]c × D[ ]d
A[ ]a × B[ ]b
Acid Base Equilibrium:
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pH = −log H3O+[ ]
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pOH = −log OH−[ ]
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Kw = H+[ ] OH−[ ] =1.0 ×10−14
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Ka =H+[ ] A−[ ]HA[ ]
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Kb =HB+[ ] OH−[ ]
B[ ]
Henderson-‐Hasselbalch Eq’n:
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pH = pKa + log baseacid⎡
⎣ ⎢ ⎤
⎦ ⎥
Electrochemistry Nernst Eq’n:
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Ecell = Ecell −
0.0592 Vn
logQ
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ΔG = −nFEcell
CONSTANTS
1 amu = 1.6605 × 10－27 kg
Avogadro’s # (NA) = 6.02214 × 1023 mol－1
Bohr radius (a0) = 5.2918 × 10－11 m
Bolzmann’s const. (k) = 1.3807 × 10-23 J/K
Faraday’s const. (F) = 9.6485 × 104 C/mol
Planck’s const. (h) = 6.6261 × 10－34 Js
Gas const. (R) = 0.0821 (Latm)/(molK)
= 8.3145 J/(molK)
Electron charge (e) = 1.6022 × 10－19 C
Mass of electron (me) = 9.1093826 × 10–31 kg
Mass of proton (mp) = 1.67262171 × 10–27 kg
Mass of neutron (mn) = 1.6749273 × 10–27 kg
Speed of light (c) = 2.9979 × 108 m/s
