CHEMISTRY FORMULAE

GASES, LIQUIDS, d = m P = pressure R, Gas constant = 8.31 joules SOLUTIONS V V = volume mole . kelvin PV = nRT T = Temperature = 0.0821 liter atm ½ ½ urms = (3kt) = (3RT) n = number of moles mole kelvin (P + n2a) (V−nb) = nRT m M d = density = 8.31 volts coulombs V2 m = mass mole kelvin 2 KEper molecule = mv v = velocity . −23 PA = Ptotal XA 2 where XA = moles A Boltzmann’s constant,k = 1.38 x 10 joule total moles K Ptotal = PA + PB + PC + KE per mole = 3RTn Kf water = 1.86 Kelvin /molal .. 2 urms = root-mean-square- Kb water = 0.512 Kelvin /molal root ½ o n = m r1 = ( M2) KE = Kinetic energy STP = 0.00 C and 1.00 atm (101.3 kpa) ½ r = rate of effusion M r2 (M1) M = Molar mass 1 faraday ℑ = 96,500 coulombs/ mole of o Kelvin = C + 273 M, molarity = moles solute π = osmotic pressure electrons liter of solution i = van’t Hoff factor P1V1 = P2V2 Kf = molal freezing point molality = moles of solute constant V1 = V2 kg of solvent Kb = molal boiling point T1 T2 constant Q = reaction quotient ΔTf = iKf • molality P1 V1 = P2 V2 I =current in amperes T1 T2 q = charge in coulombs t = time ΔTb = iKb • molality o E = standard reduction π = nRTi potential V K = equilibrium constant

ATOMIC STRUCTURE E = energy OXIDATION-REDUCTION ΔE = h ν or ΔE = h f ν = frequency or f = frequency ELECTROCHEMISTRY c = ν λ or c = f λ λ = wavelength p = momentum Q = [C]c[D]d a b λ = h v = velocity [A] [B] m v n = principal quantum number where a B + b B ⇔ c C + d D c = speed of light 3.00 x 108 m/s p = m v h = Planck’s constant = 6.63 x 10−34joule s I = q/t I = amperes, q = charge in coulombs, t = time k = Boltzmann’ constant = 1.38 x 10-23 in seconds. -18 En = −2.178 x 10 joule joule/K 2 23 o o o n Avogardor’s number = 6.02 x 10 Ecell = E cell −RT lnQ = E cell − 0.0592 log Q @ 25 C molecules/mole nℑ n e = electron charge = −1.602 x 10-19 coulomb log K = nEo 1 electron volt/atom = 96.5 x 1023 kj/mole 0.0592 1 Faraday ℑ = 96,500 coulombs/mole

CHEMISTRY FORMULAE

EQUILIBRIUM EQUILIBIRUM Kinetics Equations TERMS −14 o Kw = 1 x 10 at 25 C Ka = weak acid Ao − A = kt where Ao is initial Kb = weak base concentration or amount. + - pH = −log[H ]; pOH = −log[OH ] Kw = water Kp = gas pressure ln Ao = kt pH + pOH = 14 Kc = molar A concentration −1 pH = pKa + log [A ] 1 – 1 = kt [HA] A Ao

+ pOH = pKb + log [HB ] Ln k2 = Ea (1 − 1) [B] Ln k1 R (T1 T2) pKa = −logKa, pKb = −logKb

Δn Kp = Kc (RT) Δn = moles product gas − moles reactant gas

THERMOCHEMISTRY So = standard entropy ΔSo = ∑ΔSo products − ∑ΔSo reactants Ho = standard enthalpy Go = standard free energy o ΔHo = ∑ΔHo products − ∑ΔHo reactants E = standard reduction potential T = temperature ΔGo = ∑ΔGo products − ∑ΔGo reactants q = heat c = specific heat capacity ΔGo = ΔHo − TΔSo ΔGo = −RT lnK = −2.303 RT log K Cp = molar heat capacity at constant pressure ΔGo = −nℑEo 1 faraday ℑ = 96,500 ΔG = ΔGo + RT lnQ = ΔGo + 2.303 RT log Q coulombs/mole

c = 4.18 joule q = m c ΔT water g K

H = 330 joules for water C = ΔH f p gram ΔT Hv = 2260 joules for water q = mHf gram q = mHv.