CHEM 1202 Final Exam Study Guide PDF

CHEM 1202 Final Exam Study Guide Chapter 5 – Energy Understand Energy interacts with a matter Define Exothermic & endothermic reactions Specific heat capacity Calorimetry Calculate The amount of heat energy transferred (q) The change in heat energy for a reaction...

CHEM 1202 Final Exam Study Guide Chapter 5 – Energy Understand Energy interacts with a matter Define Exothermic & endothermic reactions Specific heat capacity Calorimetry Calculate The amount of heat energy transferred (q) The change in heat energy for a reaction (enthalpy) What you will be expected to know Concepts Relationship between EK, mass, and speed Relationship between potential energy, charge, and distance Work: both relationship between P and V, and relationship to q and E Relationship between enthalpy, energy, and P-V Endothermic and exothermic Equations and calculations q for constant pressure and constant volume calorimeter Adding reactions and adding ΔH (Hess’ law) Dimensional analysis with ΔH Using a table of ΔHof to find ΔHorxn Chapter 19 – Chemical Thermodynamics Understand – Whether a reaction occurs is determined by entropy, enthalpy, and temperature. Define – Spontaneous vs nonspontaneous processes Calculate Entropy Gibb’s free energy What you will be expected to know Concepts Spontaneity vs. reversibility Predict if S increases or decreases (microstates) based on physical state and n; V, P and T Calculations: S from q (or ΔH) and T at phase equilibrium  ΔSorxn and ΔGorxn as a summation (of So or ΔGof, respectively). ΔG as it relates to ΔH and ΔS. ΔG and ΔGo as it relates to K (and Q). Equations that you need to remember ° ° ° ∆Grxn = Σn(∆Gf,products ) − Σn(∆Gf,reactants ) ° ° ° ∆Hrxn = Σn(∆Hf,products ) − Σn(∆Hf,reactants ) ° ° ° ∆Srxn = Σn(∆Sf,products ) − Σn(∆Sf,reactants ) ∆G° = ∆H ° − T∆S ° or ∆G = ∆G° + RT ln Q ∆G° = −RT ln K or K = e−∆G°/RT Chapter 14 – Chemical Kinetics Understand Which factors affect rates and why Reaction orders Reaction mechanisms Define Rate law Intermediate and Catalyst Calculate Reaction orders Reaction constants Relative rates Half-life Activation energy What you will be expected to know Concepts Find reaction order given a data table or rate law. Know all rate laws & integrated rate laws (linear) o Zeroth order: Rate = 𝑘[A]0 = 𝑘 -> Rate is not affected by [A] o First order: Rate = 𝑘[A]1 = k[A] -> Rate will double if [A] doubles o Second order: Rate = 𝑘[A]2 -> Rate will quadruple if [A] quadruples Know what factors affect the rate of a reaction. Understand Ea graph and recognize reaction enthalpy.  Determine rate law for two-step reaction. Identify a catalyst; know its function. Calculations: Average rate (M/s) Rate or rate constant given rate law and orders o If only the rate data is given, use these equations ▪ Rate = 𝑘[A]x [B]y Rate1 Rate1 log log Rate2 Rate3 ▪ x= [A] y= [B] log 1 log 1 [A]2 [B]3 o Zeroth order ▪ Rate = 𝑘[A]0 = 𝑘 ▪ [A]t = −𝑘t + [A]0 o First order ▪ Rate = 𝑘[A]1 = 𝑘[A] ▪ ln[A]t = −𝑘t + ln[A]0 o Second order ▪ Rate = 𝑘[A]2 1 1 ▪ = +𝑘t + [A] [A]t 0 Half-life of a reaction 0.693 o t1/2 = 𝑘 Find Ea (Arrhenius equation) given k and T values, or k given Ea. Ea o 𝑘 = Ae−RT E o ln 𝑘 = − RTa + ln A Chapter 15 & Section 17.4 – Chemical Equilibrium & Solubility Equilibria Understand Equilibrium processes Factors that affect equilibria Equilibrium concepts applied to partially soluble salts. Solubility ICE tables of a partially soluble salt. Define Dynamic equilibria Reaction quotient and shifts Le Châtelier’s principle Calculate Equilibrium constants (concentration & pressure) Equilibrium concentrations (ICE tables) What you will be expected to know Concepts What is an equilibrium reaction. Understand the meaning of the Kc value. How to write Kc for a heterogeneous reaction. Predict reaction shifts with changing concentration, pressure, or temperature (relation to Q and K). Know how to write a dissociation reaction. Know how to write the Ksp equation from the dissociation reaction. Common ion effect. Calculations: KC (and KP from KC) o 𝐾𝑃 = 𝐾𝑐 (RT)Δn The value for Q, and compare to K. Use an I.C.E. table to find KC or equilibrium concentrations. Be able to find Ksp from molar solubility (and vice versa). Chapter 16 & 17 – Acid-Base Equilibria Understand Acid/base characteristics that affect reactivity Define Bronsted-Lowry acids/bases Lewis acids & bases Arrhenius acids & bases Polyprotic acids Buffer Calculate pH, pOH, pKa Titrations with weak acids & bases What you will be expected to know Concepts Definitions of Bronsted-Lowry acids and bases. Identify strong acids and strong bases. Know general dissociation reactions for weak acids and bases and from those write Ka and Kb expressions. Determine if a salt is acidic, basic, or neutral. Be able to rank acidity and basicity based on position on periodic table, electronegativity, anion’s charge, or number of O atoms.  Polyprotic acids Common ion effect Buffers, buffer range and buffer capacity. Recognize titration graphs and identify stages. Calculations: Find [H3O+] given [OH−] (and vice versa). Be able to calculate pH/pOH and pK. Find pH from concentration of acid/base (ICE table), or from Ka. Find Ka (or Kb) from pH (or pOH). Percent ionization Find Ka from Kb – or pKa from pKb (or vice versa) for conjugate pairs. pH of salt solutions Use Henderson–Hasselbalch equation in buffer calculations Titration calculations for o A strong acid and strong base o A weak acid and strong base