University:
Miami University
Course:
CHM 141 | College Chemistry
Academic year:

2020
Views:

441

Pages:

2
Author:

5prinzg1s

AP® CHEMISTRY EQUATIONS AND CONSTANTS UNIT SYMBOLS gram, mole, liter, meter, second, hertz, atmosphere, millimeter of mercury, degree Celsius, kelvin, joule, volt, coulomb, ampere, g mol L m s Hz atm mm Hg °C K J V C A UNIT CONVERSIONS 1 hertz = 1 s−1 1 atm = 760 mm Hg = 760 torr K = °C + 273.15 1 volt = 1 joule 1 coulomb 1 ampere = 1 coulomb 1 second METRIC PREFIXES Factor Prefix Symbol 109 giga G 106 mega M 103 kilo k 10−2 centi c 10−3 milli m 10−6 micro μ 10−9 nano n 10−12 pico p ATOMIC STRUCTURE E ν λ F q r E = hν c = λν Fcoulombic ∝ q1q2 r2 = = = = = = energy frequency wavelength force charge separation Planck's constant, h = 6.626 × 10−34 J s Speed of light, c = 2.998 × 108 m s−1 Avogadro's number = 6.022 × 1023 mol−1 GASES, LIQUIDS, AND SOLUTIONS PV PV 1 1 = 2 2 T1 T2 PV = nRT PA = Ptotal × X A , where X A = Ptotal = PA + PB + PC + ... n= m M D= m V KE = 1 2 mv 2 n M = solute L solution A = ε bc moles A total moles P= V = T = n= X = m= M = D= KE = v= M = A= ε = b= c= pressure volume temperature number of moles mole fraction mass molar mass density kinetic energy velocity molarity absorbance molar absorptivity path length concentration Gas constant, R = 8.314 J mol−1 K −1 = 0.08206 L atm K −1 mol−1 STP = 273.15 K and 1.0 atm Ideal gas at STP = 22.4 L mol−1 KINETICS [A]t − [A]0 = − kt k = rate constant t = time t 1 = half-life ln[A]t − ln[A]0 = − kt 2 1 1 − = kt [A]t [A]0 t1 = 2 0.693 k EQUILIBRIUM Kc = Kp = [C]c [D]d [A]a [B]b , where a A + b B  c C + d D (PC )c (PD ) d (PA ) a (PB )b + − K w = [H 3O ][OH ] = 1.0 × 10 −14 at 25°C pK w = 14 = pH + pOH at 25°C pH = − log[H 3O+ ], Kb = pK a = − log K a , pH = pK a + log (gas pressures) Kw (water) Ka (acid) Kb (base) pK w = pK a + pK b [A − ] [HA] products −∑ ∆H f reactants   ∆Sreaction = ∑ S products −∑ Sreactants products −∑ ∆G f ∆G ° = ∆H ° − T ∆S ° = − RT ln K = −nFE ° q t  − Ecell = Ecell Kp [OH − ][HB+ ] [B] THERMODYNAMICS/ELECTROCHEMISTRY q = mc∆T I = (molar concentrations) pK b = − log K b K w = K a × Kb ,  ∆Greaction = ∑ ∆G f Kc pOH = − log[OH − ] [H 3O+ ][A − ] Ka = , [HA]  = ∑ ∆H f ∆H reaction Equilibrium Constants RT ln Q nF reactants q m c T S° H° G° R K n E° I q t Q = = = = = = = = = = = = = = = heat mass specific heat capacity temperature standard entropy standard enthalpy standard Gibbs free energy gas constant equilibrium constant number of moles of electrons standard potential current (amperes) charge (coulombs) time (seconds) reaction quotient Faraday's constant, F = 96, 485 coulombs / 1 mol e−