Notes: ° denotes at standard state; Δ indicates change in; [ ] denote molar concentrations
Chapter 8 Chapter 13
2
Ek = ½mv Kc = [C]c x [D]d / [A]a x [B]b
E=w×H Kp = ([C]RT)c x ([D]RT)d / ([A]RT)a x ([B]RT)b
w=F×d Kp = (PC)c x (PB)b / (PA)a x (PB)b
ΔE = q + w Kp = Kc x (RT)Δn
ΔE = q - PΔV Qc = [C]c x [D]d / [A]a x [B]b
qv = ΔE Chapter 15
qp = ΔE + PΔV = ΔH Kw = [H3O+] x [OH-]
ΔH = Hproducts - Hreactants pH = -log [H3O+]
C = q ⁄ ΔT pOH = -log [OH-]
q = Cm x (moles) x ΔT Ka = [H30+] x [A-] / [HA]
ΔH°reaction1 + ΔH°reaction2 …= ΔH°total Percent dissociation = [HA] dissociated / [HA] initial
ΔHfusion + ΔHvap = ΔHsubl Kb = [BH+] x [OH-] / [B]
ΔH° = ΔH°f (products) - ΔH°f (reactants) Ka x Kb = Kw
ΔH° = D Chapter 16
ΔH° = D(bonds broken) - D(bonds formed) Kn = 1 / Kw
ΔS = Sfinal - Sinitial pH = -log Ka + log [base] / [acid]
ΔG = ΔH - TΔS Ksp = [Mn+]m x {Xy-]x
Chapter 9 Kf = [C]c x [D]d / [A]a x [B]b
P=F/A K = Ksp x Kf
F=mxa IP = [Ab+]t x [Cd+]t
V∝1/P Kspa = [M2+] x [H2S] / [H30+]2
V∝T Chapter 18
V∝n 1J = 1C x 1V
PV = nRT ΔG = -nFE
Ptotal = P1 + P2 + P3 ... ΔG° = -nFE°
Effusion Rate ∝ 1 / √M E°cell = E°oxidation + E°reduction
Chapter 10 ΔG = ΔG° + RT ln Q
μ=Qxr E = E° - (RT / nF x ln Q)
2
E=zxμ/r E = E° - (0.0592V / n x log Q)
log Pvap = (-ΔHvap/ 2.303 RT) + C Ecell = 0.0592V x pH + Eref
T = ΔH / ΔS (at equilibrium) E° = RT/nF x ln K
d = nλ / 2 sin Θ
Chapter 11
M = (moles solute) / (liters solution)
X = (moles component) / (total moles)
wt % = (mass component) / (total mass)
ppm = wt% x 106
ppb = wt% x 109
m = (moles solute) / (mass solvent)
Solubility = k x P
Psoln = Psolv x Xsolv
ΔPsoln = Psolv - Psoln
Ptotal = (P°AXA) + (P°BXB)
ΔTb = Kb x m
ΔTf = Kf x m
Π = MRT
Chapter 8 ppb = parts per billion
Ek = kinetic energy Tb = boiling point temperature
Ep = potential energy Tf = freezing point temperature
v = velocity Π = osmotic pressure
m = mass Chapter 13
E = energy Qc = reaction quotient
F = force Chapter 15
w = work pH = puissance d'hydrogène
d = distance pOH = puissance d'hydoxyde
P = pressure / partial pressure Chapter 16
V = volume IP = ion product
A = area M = metal
q = heat Chapter 18
qv = heat from volume n = moles of electrons transferred
qp = heat from pressure E = cell potential
H = enthalpy
C = heat capacity
T = temperature
Cm = molar heat capacity
H° = enthalpy at 1atm, 25℃, 1M (i.e. Thermodynamic Standard State)
D = bond dissociation energy
S = entropy
G = Gibb's free energy
Chapter 9
a =acceleration
M = molar mass
n = moles
Chapter 10
μ = dipole moment
Q = magnitude of charge
r = distance between charges
z = ion charge
d = distance between atomic layers
n = integer (usually 1)
Tt = triple point temperature
Pt = triple point pressure
Tc = critical temperature
Pc = critical pressure
Chapter 11
M = molarity
X = mole fraction
wt % = weight percent
m = molality
ppm = parts per million
Chapter 8
Chapter 9
R = gas constant = 0.0820578(L∙atm)/(mol∙K) = 8.31451J/(mol∙K)
Chapter 10
R = gas constant = 0.0820578(L∙atm)/(mol∙K)
Chapter 11
k = Henry's Law constant
Kb = molal boiling-point-elevation constant
Kf = molal freezing-point-depression constant
Chapter 13
Kc = equilibrium constant for molarity
Kp = equilibrium constant for partial pressures
Chapter 15
Kw = 1.0 x 10-14
Ka = acid-dissociation constant
Kb = base-dissociation constant
Chapter 16
Kn = neutralization constant
Ksp = solubility product constant
Kf = formation constant
K = equilibrium constant
Kspa = solubility product in acid constant
Chapter 18
F = faraday = 9.648531 x 104 C / mol
J = joule
C = coulomb
V = volt
R = gas constant = 8.31451J/(mol∙K)
Chapter 8
ΔE = q - PΔV
ΔH = Hproducts - Hreactants
C = q ⁄ ΔT
q = Cm x (moles) x ΔT
ΔH°reaction1 + ΔH°reaction2 …= ΔH°total
ΔH° = ΔH°f (products) - ΔH°f (reactants)
ΔH° = D(bonds broken) - D(bonds formed)
ΔS = Sfinal - Sinitial
ΔG = ΔH - TΔS
Chapter 9
V∝1/P
V∝T
V∝n
PV = nRT
Ptotal = P1 + P2 + P3 ...
Effusion Rate ∝ 1 / √M
Chapter 10
log Pvap = (-ΔHvap/ 2.303 RT) + C
Chapter 11
M = (moles solute) / (liters solution)
X = (moles component) / (total moles)
wt % = (mass component) / (total mass)
ppm = wt% x 106
ppb = wt% x 109
m = (moles solute) / (mass solvent)
Solubility = k x P
Psoln = Psolv x Xsolv
ΔPsoln = Psolv - Psoln
Ptotal = (P°AXA) + (P°BXB)
Π = MRT
Chapter 13
Kc = [C]c x [D]d / [A]a x [B]b
Kp = (PC)c x (PB)b / (PA)a x (PB)b
Kp = Kc x (RT)Δn
Qc = [C]c x [D]d / [A]a x [B]b
Chapter 15
Kw = [H3O+] x [OH-]
pH = -log [H3O+]
pOH = -log [OH-]
Ka = [H30+] x [A-] / [HA]
Percent dissociation = [HA] dissociated / [HA] initial
Kb = [BH+] x [OH-] / [B]
Ka x K b = K w
Chapter 16
Kn = 1 / K w
pH = -log Ka + log [base] / [acid]
Ksp = [Mn+]m x {Xy-]x
Kspa = [M2+] x [H2S] / [H30+]2
Chapter 18
ΔG = -nFE
E°cell = E°oxidation + E°reduction
ΔG = ΔG° + RT ln Q
E = E° - (RT / nF x ln Q)
E = E° - (0.0592V / n x log Q)
Ecell = 0.0592V x pH + Eref
E° = RT/nF x ln K