Chem 401 Equation/Data Sheet L. Nuss Given information: Useful Constants and Formulas
Universal gas constant: R = 0.08206 L atmmol K
= 8.314
Jmol K
2a
4acbbx2
Boltzmann constant: k = 1.38 x 10–23
JK
Plank’s Constant: h = 6.626 x 10-34 J s
Faraday Constant: F = 9.65 x 104 C/mol e–
1 MeV = 1.602 x 10-13 J Speed of light: c = 2.998 x 108 m/s
If: ln y = x log y = x ym = x y = ex y = 10x m = log x/logy
Thermodynamics
E = q + w w = pV qsystem + qsurr = 0 G = nGproducts - mGreactants G = H - TS H = nHproducts - mHreactants Grxn = Grxn + RT ln Q S = nSproducts - mSreactants G = -RT ln K
S = k ln W fus
fusfus T
HS
vap
vapvap T
HS
S >q/T for spontaneous process
Kinetics
t
productsΔcoeff
1t
reactantsΔcoeff
1- rate Avg
Integrated rate laws:
1st order: ln
[A]t[A]0
= – kt OR ln[A]t = -kt + ln[A]o OR [A]t = [A]o e–kt
2nd order: 1/[A]t = kt + 1/[A]o 3rd order: 1/[A]t2 = kt +1/[A]o
2 zero order: [A]t = – kt + [A]o
1st Order: kk693.02lnt
21 2nd Order: t1/ 2
1k A 0
zero order: k
t2A][ 0
2/1
Arrhenius Equation: k = Ae–Ea/RT OR ATR
Ek a ln1ln
OR
12
a
1
212 T
1T1
RElnlnln
kkkk
Equilibrium
121
212 T
1T1
RH
KKlnlnKlnK
van’t Hoff equation
RSRxnRxn
T1
RHlnK
ba
dc
BADCKc nRTKcKp
Acid & Bases
Kw = [H3O+][OH-] = 1 x 10-14 pH = -log[H3O+] [H3O+]=10-pH pH + pOH = 14
Chem 401 Equation/Data Sheet L. Nuss Acid/Bases Equilibria
HA
AHHA
AOHKa
3 (Ka)(Kb) = Kw acidbasepKpH a log (Henderson-Hasselbalch Equ.)
Solubility & Complex Ion Equilibria
Ksp =[cation]c[anion]a where c = cation coefficient and a = anion coefficient
Kf = [complex ion]/[cation][ligand] Kd = 1/Kf Electrochemistry
Wmax=-nFEcell Ecell = oxidation potential + reduction potential Ecell = Ecathode + (-Eanode)
G°rxn = –RT ln K = –nFE°cell K logn
0.0592 logK nF
2.303RTlnKnFRTEcell
Ecell = E°cell – nFRT
ln Q OR QlognF
RT303.2EE cellcell (Nernst Equation)
Coulombs = amperes x seconds Volt = Joule / Coulomb Nuclear Chemistry
Rate = kNt k0.693t1/2 tk
NNln
0
t 2A
2B
B
A
dd
II
After decay amount = (original amount)(1/2)n before decay amount = (end amount)(2)n
E = mc2 (mass in kg, speed of light in m/s) E = (m)c2
Transition Metal Chemistry
E = Δ = h = hc/ ( in m, h = 6.62610–34 J•s)
Spectrochemical Series: Weak field ligands strong field ligands I-< Br- < S2- < :SCN- < Cl- < F- < OH– < C2O4
2– < :ONO– < H2O < :NCS– < EDTA4- < NH3 < en < phen < :NO2– < CN– ≈ CO
Crystal field Splitting of d orbitals:
octahedral tetrahedral square planar
dxy dyz
d
dxy dyz
d
dxy
800 nm
red
400 nm
orange yellow
green
violet blue
650 nm
600 nm
560 nm
490 nm
430 nm
At 25 °C
Chem 401 Equation/Data Sheet L. Nuss
B. Selected Thermodynamic Quantities for Selected Substances at 25C
Chem 401 Equation/Data Sheet L. Nuss
C. Aqueous Equilibrium Constants
1. Dissociation Constants at 25C
Chem 401 Equation/Data Sheet L. Nuss
2. Dissociation Constants for Hydrated Metal Ions at 25C
3. Dissociation constants for Bases at 25C
4. Solubility Product constants for Compounds at 25C