University:
University of Arizona
Course:
CHEM 141 | General Chemistry Lecture I
Academic year:

2022
Views:

463

Pages:

1
Author:

Lance Gutierrez

General Chemistry II Equation Sheet Think about how to set up the problem first, then apply the needed principles and formulas. Phase Changes Acids and Bases Kw = [H3 O+ ][OH − ] = Ka × Kb ∆Tb = iKb m pOH = − log[OH − ] ∆Tf = iKf m π = iMRT [OH − ] = 10−pOH c = kP pH + pOH = pKa + pKb = 14.00 (at 25◦ C) Psolution = χsolvent P ◦ pH = pKa + log solvent ∆P = P ◦ solvent − Psolution = χsolute P ◦ solvent pOH = pKb + log [BH + ] [B] [H3 O+ ]eq [HA]0 % ionization Cells [A− ] [HA] × 100% pKa = − log(Ka ) E = E◦ − ◦ E=E − RT nF ln(Q) 0.0592 log(Q) n pKb = − log(Kb ) (at 25◦ C) Kb = 10−pKb ∆G = −nF Ecell ∆G◦ = −nF E ◦ E ◦cell = RTnF cell ln(K) E ◦cell = 0.0592V n Ka = 10−pKa Equilibria log(K) (at 25◦ C) [C]c [D]d [A ]a [B ]b Qc = [C]c [D]d [A]a [B]b Kc = USE ONE: E ◦cell = E ◦ cathode(red.) − E ◦ anode(red.) Qp = E ◦cell = E ◦ cathode(red.) + E ◦ anode(red.) Kp = P d D ·P cC P aA ·P bB Pd c D ·P C PAa ·P bB Kp = Kc [R × T ]∆n Thermodynamics ∆G = ∆G◦ + RT ln(Q) ∆G = ∆H − T ∆S ∆G◦ = −RT ln(K ) ∆Ssurr = −∆Hsys rate = k[A]x [B ]y T k = Ae− ∆Suniv = ∆Ssys + ∆Ssurr ∆S ◦rxn = ΣS ◦ products + ΣS ◦ ∆G◦rxn = Σ∆G◦ products + ln( reactants Σ∆G◦ reactants k1 Ea k2 ) RT = half life = Ea R ( T12 − 1 T1 ) ln(2) k [A]t = −kt + [A]o Concentrations ln([A]t ) = −kt + ln([A]o ) molessolute molality = mass solvent(kg ) solute % by mass = masssolutemoles +masssolvent 1 [A]t × 100% = kt + 1 [A]o