AP Chemistry Equations and Constants Cheat Sheet, Cheat Sheet of Chemistry

Download AP Chemistry Equations and Constants Cheat Sheet and more Cheat Sheet Chemistry in PDF only on Docsity! ADVANCED PLACEMENT CHEMISTRY EQUATIONS AND CONSTANTS Throughout the test the following symbols have the definitions specified unless otherwise noted. L, mL = liter(s), milliliter(s) mm Hg = millimeters of mercury g = gram(s) J, kJ = joule(s), kilojoule(s) nm = nanometer(s) V = volt(s) atm = atmosphere(s) mol = mole(s) ATOMIC STRUCTURE E = hν c = λν E = energy ν = frequency λ = wavelength 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 Electron charge, e = −1.602 × 10−19 coulomb EQUILIBRIUM Kc = [C] [D] [A] [B] c d a b , where a A + b B c C + d D Kp = C A B ( ) ( ) ( ) ( ) c d D a b P P P P Ka = [H ][A ] [HA] + - Kb = [OH ][HB ] [B] - + Kw = [H +][OH−] = 1.0 × 10−14 at 25°C = Ka × Kb pH = − log[H+] , pOH = − log[OH−] 14 = pH + pOH pH = pKa + log [A ] [HA] - pKa = − logKa , pKb = − logKb Equilibrium Constants Kc (molar concentrations) Kp (gas pressures) Ka (weak acid) Kb (weak base) Kw (water) KINETICS ln[A] t − ln[A]0 = − kt [ ] [ ]0A A 1 1 t - = kt t½ = 0.693 k k = rate constant t = time t½ = half-life ADVANCED PLACE ENT C E ISTRY E UATI NS AND C NSTANTS Throughout the test the fol owing sy bols have the definitions specified unless otherwise noted. L, L = liter(s), il iliter(s) Hg = il i eters of ercury g = gra (s) J, kJ = joule(s), kilojoule(s) n = nano eter(s) V = volt(s) at = at osphere(s) ol = ole(s) AT IC STRUCTURE E = hν c = λν E = energy ν = frequency λ = wavelength Planck’s constant, h = 6.626 × 10−34 J s Speed of light, c = 2.998 × 108 s−1 Avogadro’s nu ber = 6.022 × 1023 ol−1 Electron charge, e = −1.602 × 10−19 coulo b E UILIBRIU Kc = [C] [D] [A] [B] c d a b , where a A + b B c C + d D Kp = C A B ( ) ( ) ( ) ( ) c d D a b P P P P Ka = [H ][A ] [HA] + - Kb = [OH ][HB ] [B] - + Kw = [H +][OH−] = 1.0 × 10−14 at 25°C = Ka × Kb pH = − log[H+] , pOH = − log[OH−] 14 = pH + pOH pH = pKa + log [A ] [HA] - pKa = − logKa , pKb = − logKb Equilibriu Constants Kc ( olar concentrations) Kp (gas pressures) Ka (weak acid) Kb (weak base) Kw (water) INETICS ln[A] t − ln[A]0 = − kt [ ] [ ]0A A 1 1 t - = kt t = 0.693 k k = rate constant t = ti e t = half-life GASES, LIQUIDS, AND SOLUTIONS PV = nRT PA = Ptotal × XA, where XA = moles A total moles Ptotal = PA + PB + PC + . . . n = m M K = °C + 273 D = m V KE per molecule = 1 2 mv2 Molarity, M = moles of solute per liter of solution A = abc 1 1 pressure volume temperature number of moles mass molar mass density kinetic energy velocity absorbance molarabsorptivity path length concentration Gas constant, 8.314 J mol K 0.08206 P V T n m D KE A a b c R Ã - - = = = = = = = = = = = = = = = M 1 1 1 1 L atm mol K 62.36 L torr mol K 1 atm 760 mm Hg 760 torr STP 0.00 C and 1.000 atm - - - -= = = = THERMOCHEMISTRY/ ELECTROCHEMISTRY products reactants products reactants products reactants ln ff ff q mc T S S S H H H G G G G H T S RT K n F E q I t D D D D D D D D D D D = = -Â Â = -Â Â = -Â Â = - = - = -  heat mass specific heat capacity temperature standard entropy standard enthalpy standard free energy number of moles standard reduction potential current (amperes) charge (coulombs) t q m c T S H G n E I q t = = = = = = = = = = = = ime (seconds) Faraday’s constant , 96,485 coulombs per mole of electrons 1 joule 1volt 1coulomb F = =