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### Che 107 Objectives

Course: CHE 107, Spring 2008
School: Jefferson Community and...
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Concept All Areas for Che 107 (all fair game on final) Chapter 14: Solutions and Their Behavior Concept Area I: Terminology Molarity, M molality, m mole fraction, X solution solvent solute colligative properties weight percent parts per million, ppm saturated solubility miscible immiscible hydrated heat of solution Henry's law Raoult's law ideal solution molal boiling point elevation constant molal freezing point...

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Coursehero >> Kentucky >> Jefferson Community and Technical College >> CHE 107

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Concept All Areas for Che 107 (all fair game on final) Chapter 14: Solutions and Their Behavior Concept Area I: Terminology Molarity, M molality, m mole fraction, X solution solvent solute colligative properties weight percent parts per million, ppm saturated solubility miscible immiscible hydrated heat of solution Henry's law Raoult's law ideal solution molal boiling point elevation constant molal freezing point depression constant van't Hoff factor, i colloids emulsion Concept Area II: Units of Concentration a. You should remember the definition of Molarity, M, and be able to use Molarity in calculations. b. You should know the definition of molality, m, and be able to use molality in calculations. c. You should know the definition of a mole fraction, X, and be able to use mole fractions in calculations. d. You should know the definition of percent by mass or parts per million, ppm, and be able to use both in calculations. Concept Area III: Solutions and Suspensions a. You should remember what the terms solution, solvent and solute mean. b. You should understand the distinctions between saturated, unsaturated and supersaturated solutions. c. You should be able to tell the difference between homogenous solutions, heterogeneous solutions, suspensions, and colloids. d. You should be able to describe the effect of pressure and temperature on the solubility of a solid in a liquid solvent. Concept Area IV: Heat of Solution a. You should be able to describe the process of dissolving a solute in a solvent including the energy changes that may occur. b. You should be able to relate lattice energy and enthalpy of hydration to the enthalpy of solution for an ionic solute. Concept Area V: Gases in Solution a. You should qualitatively understand Henry's Law. b. You should be able to describe the effect of pressure and temperature on the solubility of a gas in a liquid solvent. Concept Area VI: Colligative Properties a. You should know what colligative properties are and be able to give some examples. b. You should be able to calculate the mole fraction of a solute or solvent and tell the effect of adding a solute (molecular or ionic) on the solvent's vapor pressure using Raoult's law for ideal solutions. c. You should be able to calculate the boiling point elevation or the freezing point depression caused by a solute (molecular or ionic) in a solvent for ideal solutions. d. You should be able to use colligative properties to determine the Molar mass of a solute. Che 107 Objectives.doc Page 1 of 10 All Concept Areas for Che 107 (all fair game on final) Chapter 16: Principles of Reactivity: Chemical Equilibria Concept Area I: Terminology kinetics chemical equilibrium dynamic equilibrium homogeneous equilibrium heterogeneous equilibrium reaction quotient, Qc equilibrium constant, Kc or Keq equilibrium constant expression Le Chtelier's Principle Concept Area II: Introduction to Chemical Equilibrium a. You should be able to distinguish the difference between the rate and the extent of a reaction. b. You should understand the difference between the kinetic and equilibrium region on a graph of concentration of products and reactant versus time. c. You should know that an equilibrium condition will be reached no matter the starting conditions. d. You should realize that at equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction. e. You should remember that we use the following arrow for chemical reactions at equilibrium: . Concept Area III: Q and K a. You should know how to write a Q/K from a balanced chemical equation. b. You should understand that at equilibrium Q = K. c. You should know that the magnitude of Q indicates which way the reaction must go to reach equilibrium. d. You should realize that the magnitude of K tells whether mostly products or reactants are present at equilibrium. e. You should be able to explain why pure liquids and solids do not appear in a Q/K. f. You should know how to solve equilibrium problems using the quadratic formula when appropriate. Concept Area IV: Le Chtelier's Principle a. You should know what the Le Chtelier's Principle is and how to apply it. b. You should be able to use Le Chtelier's Principle to predict which way the equilibrium will shift (if it will shift at all) if a stress is applied. Che 107 Objectives.doc Page 2 of 10 All Concept Areas for Che 107 (all fair game on final) Chapter 17: Principles of Reactivity: Chemistry of Acids and Bases Concept Area I: Terminology ionization constant, Ka or Kb water ionization constant, Kw pH pOH Arrhenius acid Arrhenius base Brnsted-Lowry acid Brnsted-Lowry base Lewis acid Lewis base strong/weak acids & bases monoprotic acid diprotic acid triprotic acid polyprotic acid aprotic amphoteric conjugate acid-base pair autoionization complex ion Concept Area II: Reintroduction to Acids and Bases a. You should still know the strong acids and bases learned in CHE 105. b. You should know the difference between Arrhenius, Brnsted-Lowry and Lewis definitions of acids and bases. c. You should be able to recognize acids/bases and be able to tell which definition(s) they meet. d. You should be able to write an acid-base reaction and describe the result. e. You should be able to label conjugate acid-base pairs in an acid-base reaction. f. You should be able to tell whether an acid is monoprotic, diprotic and so on. g. You should understand what an amphoteric compound is and be able to recognize one. Concept Area III: pH and pOH a. You should remember (from CHE 105) how to use and understand the pH scale (this includes calculating pH from H+ and H+ from pH). b. You should be able to use and understand the pOH scale (this includes calculating pOH from OH and OH from pOH). c. You should be able to convert between the pH and the pOH scales. Concept Area IV: Kw a. You should remember the concept of water autoionization from CHE 105. b. You should know and be able to use the water ionization constant, Kw. Concept Area V: Ka and Kb a. You should be able to write equilibrium constant expressions for acids and bases. b. You should understand the relationhsip between Ka for a weak acid to its Kb for its conjugate base and vice versa. c. You should be able to solve acid-base equilibrium problems. Concept Area VI: pKa and pKb a. You should be able to calculate the pKa or pKb from the Ka or Kb and vice versa. b. You should understand how pKa and pKb is correlated with acid and base strength. c. You should be able to describe the acid-base properties of the salts of acids and bases. d. You should be able to calculate the pH or pOH of a solution of a salt of a weak acid or a weak base. e. You should be able to calculate the pH or pOH after any acid-base reaction. Che 107 Objectives.doc Page 3 of 10 All Concept Areas for Che 107 (all fair game on final) Chapter 18: Principles of Reactivity: Other Aspects of Aqueous Equilibria Concept Area I: Terminology common ion effect buffer Henderson-Hasselbalch equation titrant titration acid-base indicator insoluble solubility product constant, Ksp complex ion formation constant, Kform Concept Area II: The Common Ion Effect a. You should understand what the common ion effect is. b. You should be able to predict qualitatively and quantitatively the effect of the addition of a "common ion" on the pH of a solution of a weak acid or base. Concept Area III: Buffers a. You should know what a buffer solution is and be able to describe how to make one. b. You should be able to calculate the pH of a buffer system under different conditions. Concept Area IV: Acid-Base Titrations a. You should remember how to calculate the pH or pOH after any acid-base reaction. b. You should be able to calculate what the pH will be at the equivalence point for a titration between any acid and base. c. You should understand the differences between the titration curves for strong vs. strong, strong vs. weak and weak vs. weak. d. You should be able to describe how an indicator is used in an acid-base titration. Concept Area V: Solubility Product Constant, Ksp, and the Formation Constant, Kform a. You should be able to write the equilibrium constant expression for any insoluble salt. b. You should understand how Ksp is correlated with the salt's solubility. c. You should be able to solve calculations involving Ksp including deciding whether or not a precipitate will form under given conditions. d. You should be able to calculate the solubility of a salt in the presence of a common ion. e. You should understand that the formation of a complex ion can cause more of an insoluble salt to dissolve. f. You should be able to use equilibrium constants to devise a separation scheme for various ions. Che 107 Objectives.doc Page 4 of 10 All Concept Areas for Che 107 (all fair game on final) Chapter 6 Principles of Reactivity: Energy and Chemical Reactions Concept Area I: Terminology calorie, c Calorie, C calorimetry energy enthalpy, H enthalpy change, H endothermic exothermic heat internal energy, E or U joules, J kinetic energy molar heat capacity potential energy standard enthalpy of formation standard state state function specific heat surroundings system temperature thermodynamics latent heat (phase changes) work Concept Area II: Heat and Energy a. You should be able to describe the various forms of energy (i.e. kinetic energy and potential energy) and give examples in which one is converted to the other. b. You should still be able to differentiate between heat and temperature. c. You should be able to use joules or calories and know that 4.184 J = 1 cal. d. You should understand what is meant by a state function and by standard state. Concept Area III: First Law of Thermodynamics a. You should be able to state the First Law of Thermodynamics and relate it to a series of energy changes. b. You should recognize that when a process is carried out under constant pressure conditions, the heat transferred is the enthalpy change. c. You still be able to define change in enthalpy, H, mathematically (H = Hproducts Hreactants) and determine if a reaction is exothermic or endothermic. d. You should understand the difference between the system and the surroundings. e. You should be able to draw and interpret energy level diagrams for a chemical f. reaction. You should be able to do stoichiometric calculations involving the use of enthalpy. Concept Area IV: Calculating Energy Changes in Reactions a. You should be able to describe how to measure the quantity of heat energy transferred in a reaction by using calorimetry. b. You should be able to apply Hess's law to find the enthalpy change for a reaction. c. You should be able to use standard molar enthalpy of formation, Hf, to calculate the enthalpy change for a reaction, Hrxn. d. You should be able to calculate Hrxn from bond dissociation energies. Che 107 Objectives.doc Page 5 of 10 All Concept Areas for Che 107 (all fair game on final) Chapter 19: Principles of Reactivity: Entropy and Free Energy Concept Area I: Terminology spontaneous entropy, S standard entropy, S second law of thermodynamics third law of thermodynamics Gibbs free energy, G standard free energy of formation, Gf Concept Area II: Entropy a. You should understand that entropy is a measure of disorder. b. You should recognize that entropy can be determined experimentally as the heat change of a reversible process. c. You should know how to calculate entropy changes. d. You should be able to identify common processes that are entropy-favored. Concept Area III: Will a process be spontaneous? a. You should be able to use entropy and enthalpy changes to predict whether a reaction is spontaneous or not. b. You should understand the roll of temperature on whether a reaction is spontaneous or not. Concept Area IV: Gibbs Free Energy a. You should know how entropy changes, enthalpy changes and temperature can be used to calculate the Gibbs free energy for a process. b. You should understand how a change in temperature changes the Gibbs free energy of a process. c. You should be able to calculate the standard free energy of formation from standard entropy and enthalpy values or from standard free energy values. Concept Area V: Application of Thermodynamics to Equilibrium a. You should be able to describe the relationship between the free energy change and equilibrium constants. b. You should be able to calculate equilibrium constants from Grxn. Che 107 Objectives.doc Page 6 of 10 All Concept Areas for Che 107 (all fair game on final) Chapter 15: Principles of Reactivity: Chemical Kinetics Concept Area I: Terminology chemical kinetics reaction mechanism rate of reaction instantaneous rate rate equation rate law rate constant order of reaction initial rate integrated rate equation half-life, t collision theory activation energy, Ea Arrhenius equation intermediate elementary step molecularity unimolecular bimolecular rate-determining step Concept Area II: Collision Theory and Activation Energy a. You should be able to list the factors that affect the speed of a chemical reaction. b. You should be able to describe the collision theory of reaction rates. c. You should be able to use collision theory to describe the effect of reactant concentration, molecular orientation, temperature, and speed on the reaction rate. d. You should be able to relate activation energy to the rate and thermodynamics of a reaction using reaction coordinate diagrams. e. You should know what a catalyst is and what it does to the rate of a chemical reaction. Concept Area III: Rates of Reaction and Introduction to Rate Laws a. You should be able to explain the concept of reaction rate and know how to determine it. b. You should be able to derive instantaneous rates of reaction from experimental information. c. You should be able to interpret a reaction rate in terms of reactant and product concentrations. d. You should know what a rate law equation looks like and be able to define various parts of it. e. You should understand what is meant by the reaction order and be able to give the reaction order for any reactant or for the overall equation. Concept Area IV: Deriving Information from Experimental Data a. You should be able to derive a rate equation and the value of the rate constant from experimental information. b. You should be able to tell the order of a reaction by the units on k. Concept Area V: Integrated Rate Laws a. You should be able to describe and use the relationships between reactant concentration and time for zero, first and second-order reactions. b. You should be able to apply graphical methods for determining reaction order and the rate constant from experimental data. c. Use the concept of half-life, especially for first-order reactions. Concept Area VI: The Arrhenius Equation a. You should be able to describe the effect of temperature on the reaction rate using the Arrhenius equation. b. You should be able to use the Arrhenius equation to calculate the activation energy from experimental data. Concept Area VII: Reaction Mechanisms and Rate Laws a. You should understand the concept of a reaction mechanism. Che 107 Objectives.doc Page 7 of 10 All Concept Areas for Che 107 (all fair game on final) b. You should be able to describe the elementary steps of a mechanism and give their molecularity. c. You should be able to recognize the rate-determining step in a mechanism and identify any reaction intermediates. d. You should understand how a catalyst can change the mechanism of a reaction. e. You should now fully understand and be able to label a reaction coordinate diagram. Chapter 20: Principles of Reactivity: Electron Transfer Reactions Concept Area I: Terminology oxidation reduction oxidized reduced oxidizing agent reducing agent oxidizer reducer voltaic or galvanic cells electrolytic cells electrolysis half-reactions salt bridge anode cathode battery fuels cells electromotive force, emf standard conditions standard potential standard hydrogen electrode, SHE Nernst equation Faraday constant ion-selective electrodes Concept Area II: Electron Transfer Reactions a. You should remember how to recognize a redox reaction, and you should remember the various terms used to describe the chemicals involved in a redox reaction. b. You should be able to balance equations for oxidation-reduction reactions in acidic or basic solutions using the half-reaction approach. c. You should be able to identify the half-reactions occurring at the anode an...

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Mathematics 373 Workshop 5 Solutions Extrapolation Fall 2003Problem 11a Statement 1a SolutionWe give a rigorous derivation of a numerical differentiation formula with error term.Expand the divided difference f [x, x, y, z] to get its value in
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Mathematics 373 Workshop 6 Solutions Integration Fall 2003Problem 1.formOn the interval [-1, 1] and expressed in terms of averages, Simpson's rule has the 1 21 -1f (t) dt =f (-1) + 4 f (0) + f (1) 1 (4) - f ( ) 6 180Check this formula usi
Rutgers - MATH - 373
Mathematics 373 Workshop 7 Solutions Summation Fall 2003Introduction. In this workshop, the Euler-Maclaurin summation formula will be derived. We have seen that formulas can be derived for a standard interval which is then rescaled to apply to othe