AP Chemistry Practice Problems Module 9: Kinetics and Equilibrium

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1 AP Chemistry Practice Problems Module 9: Kinetics and Equilibrium The headings on these problems correspond to the headings on your content pages. You should work on these throughout the unit. Be sure to show all your work, otherwise you won t know where you went wrong if you made a mistake. Many times it is easier to write out your work using pen and paper, so you may choose to scan your work if you like. Just make sure that it is clear enough for me to see! Scanned work should be saved as one pdf file. Multiple files may be too large for the dropbox. If you type your answers, use a different color font, highlight, textbox, etc. to make the work easier to see. Place the completed document into the Module 9: Kinetics and Equilibrium Practice Problems dropbox according to your schedule. Kinetics, Collision Theory, Potential Energy Diagrams 1. What two factors influence the effectiveness of molecular collisions in producing chemical change? 2. Suppose we compared two reactions, one requiring the simultaneous collision of three molecules and the other requiring a collision between two molecules. From the standpoint of statistics, and all other factors being equal, which reaction should be faster? Explain your answer. 3. Many reactions that have large, negative values of G are not actually observed to happen at 25 C and 1 atm.why? Factors Affecting Reaction Rates, Chemical Nature of Reactants, Ability of the Reactants to Collide with Each Other, Concentration of the Reactants, Temperature, Presence of a Catalyst, Reaction Mechanisms 4. The rate of hardening of epoxy glue depends on the amount of hardener that is mixed into the glue. What factor affecting reaction rates does this illustrate? 5. A Polaroid instant photograph develops faster if it s kept warm than if it is exposed to cold. Why? 6. In cool weather, the number of chirps per minute from crickets diminishes. How can this be explained?

2 For the following set of questions, you can check your answers here. You can either type your answers below or take a screenshot of your completed page and insert it into the document you submit. Use this energy diagram to answer these questions. 1. The heat content of the reactants of the forward reaction is about kilojoules. 2. The heat content of the products of the forward reaction is about kilojoules. 3. The heat content of the activated complex of the forward reaction is about kilojoules. 4. The activation energy of the forward reaction is about kilojoules. 5. The heat of reaction (ΔH) of the forward reaction is about kilojoules. 6. The forward reaction is (endothermic or exothermic). 7. The heat content of the reactants of the reverse reaction is about kilojoules. 8. The heat content of the products of the reverse reaction is about kilojoules. 9. The heat content of the activated complex of the reverse reaction is about kilojoules. 10. The activation energy of the reverse reaction is about kilojoules. 11. The heat of reaction (ΔH) of the reverse reaction is about kilojoules. 12. The reverse reaction is (endothermic or exothermic). Measuring Reaction Rate, Rate Laws, Rate Laws and Reaction Mechanisms, Order of Reaction 7. For the reaction 2A + B 3C, it was found that the rate of disappearance of B was 0.30 mol L 1 s 1. What is the rate of disappearance of A and the rate of appearance of C? 8. A reaction has the following rate law: What are the units of the rate constant, k? 9. A reaction has the following mechanism: What is the net overall change that occurs in this reaction?

3 10. Estimate the rate of the reaction given that the rate law for the reaction is for neutral water where [H + ] = M and [OH ] = M. 11. The rate law for the decomposition of N 2 O 5 is If k = s 1, what is the reaction rate when the N 2 O 5 concentration is mol L 1? 12. For the reaction the rate law is rate = k [HCrO 4 ] [HSO 3 ] 2 [H + ]. a. What is the order of the reaction with respect to each reactant? b. What is the overall order of the reaction? 13. A key elementary process in the destruction of stratospheric ozone from nitrogen oxides in jet exhaust is the reaction The rate law is rate = k [NO][O 3 ]. a. What is the order with respect to each reactant? b. What is the overall order of the reaction? 14. Cyclopropane, C 3 H 6, is a gas used as a general anesthetic. It undergoes a slow molecular rearrangement to propylene. At a certain temperature, the following data were obtained relating concentration and rate. Initial Concentration of Rate of Formation of C 3 H 6 (mol L 1 ) Propylene (mol L 1 s 1 ) What is the rate law for the reaction? What is the value of the rate constant, with correct units? 15. The formation of small amounts of nitric oxide, NO, in automobile engines is the first step in the formation of smog. As noted earlier, nitric oxide is readily oxidized to nitrogen dioxide by the reaction 2NO + O 2 2NO 2 The following data were collected in a study of the rate of this reaction. Initial Concentrations (mol L 1 ) [O 2 ] [NO] Rate of Formation of NO 2 (mol L 1 s 1 ) What is the rate law for the reaction? What is the rate constant with its correct units?

4 16. At a certain temperature the following data were collected for the reaction 2ICl + H 2 I 2 + 2HCl. Initial Concentrations (mol L 1 ) [ICl] [H 2 ] Initial Rate of Formation of I 2 (mol L 1 s 1 ) Determine the rate law and the rate constant (with correct units) for the reaction. 17. The following data were obtained for the reaction of (CH 3 ) 3 CBr with hydroxide ion at 55 C. (CH 3 ) 3 CBr + OH- (CH3)3COH + Br- Initial Concentrations (mol L 1 ) [(CH 3 ) 3 CBr] [OH ] Initial Rate of Formation of (CH 3 ) 3 COH (mol L 1 s 1 ) What is the rate law for the reaction? What is the value of the rate constant (with correct units) at this temperature? Integrated Rate Laws, Half Life, Activation Energy 18. The decomposition of SO 2 Cl 2 described in Problem has a first- order rate constant k = s 1 at 320 C. If the initial SO 2 Cl 2 concentration in a container is M, what will its concentration be (a) after 1.00 hour, (b) after 1.00 day? 19. If it takes 75.0 min for the concentration of a reactant to drop to 20% of its initial value in a first- order reaction, what is the rate constant for the reaction in the units min 1? 20. The decomposition of hydrogen iodide follows the equation 2HI(g) H 2 (g) + I 2 (g). The reaction is second order and has a rate constant equal to L mol 1 s 1 at 700 C. If the initial concentration of HI in a container is M, how many minutes will it take for the concentration to be reduced to M? 21. The second- order rate constant for the decomposition of HI at 700 C was given in the preceding problem. At min after a particular experiment had begun, the HI concentration was equal to mol L 1. What was the initial molar concentration of HI in the reaction vessel? 22. What is meant by the term half- life? 23. Strontium- 90 has a half- life of 28 years. How long will it take for all of the strontium- 90 presently on Earth to be reduced to 1/32nd of its present amount? 24. The decomposition of NOCl, the compound that gives a yellow- orange color to aqua regia (a mixture of concentrated HCl and HNO 3 that's able to dissolve gold and platinum) follows the reaction 2NOCl 2NO + Cl 2. It is a second- order reaction with k = L mol 1 s 1 at 400 K. What is the half- life of this reaction if the initial concentration of NOCl is 0.20 mol L 1?

5 Dynamic Equilibrium, Equilibrium Law 25. Write the equilibrium law for each of the following gaseous reactions in terms of molar concentrations: a. 3Cl 2 (g) + NH 3 (g) NCl 3 (g) + 3HCl(g) b. PCl 3 (g) + PBr 3 (g) PCl 2 Br(g) + PClBr 2 (g) 26. Write the equilibrium law for the following reaction in aqueous solution: HClO(aq) + H 2 O H 3 O + (aq) + ClO (aq) 27. Write the equilibrium law corresponding to K c for each of the following heterogeneous reactions: a. CaCO 3 (s) + SO 2 (g) CaSO 3 (s) + CO 2 (g) b. AgCl(s) + Br (aq) AgBr(s) + Cl (aq) 28. Use the following equilibria: to calculate K c for the reaction The Meaning of Kc, Determining Kc from Other Reactions, Kc and Kp 29. Here are some reactions and their equilibrium constants: (a) 2CH 4 (g) C 2 H 6 (g) + H 2 (g) Kc = 9.5 x (b) CH 3 OH(g) + H 2 (g) CH 4 (g) + H 2 O(g) Kc = 3.6 x (c) H 2 (g) + Br 2 (g) 2HBr(g) Kc = 2.0 x 10 9 Arrange these reactions in order of their increasing tendency to go toward completion. 30. For a specific reaction, which of the following statements can be made about the equilibrium constant? a. it can change with temperature b. it may be changed by addition of a catalyst c. it increases if the concentration of one of the products is increased d. it increases if the concentration of one of the products is decreased e. it always remains the same 31. State the equation relating KP to Kc and define all terms. Which is the only value of R that can be properly used in this equation? ( ) Δn g K p = K c RT 32. The reaction CO(g) + 2 H 2 (g) CH 3 OH(g) has K P = at 225 C. What is the value of K c at this temperature? Predicting Changes in Equilibrium, Adding or Removing a Reactant or Product, Changing the Volume of a Gaseous System, Addition of an Inert Gas, Changing the Temperature of a System, Adding a Catalyst 33. How will the equilibrium be affected by the following? a. The addition of CH 4 (g)

6 b. The addition of H 2 (g) c. The removal of CS 2 (g) d. A decrease in the volume of the container e. An increase in temperature 34. The reaction CO(g) + 2 H 2 (g) CH 3 OH(g) has ΔH = 18 kj. How will the amount of CH 3 OH present at equilibrium be affected by the following? a. Adding CO(g) b. Removing H 2 (g) c. Decreasing the volume of the container d. Adding a catalyst e. Increasing the temperature 35. Consider the equilibrium In which direction will this equilibrium be shifted by the following changes? a. Addition of N 2 O b. Removal of NO 2 c. Addition of NO d. Increasing the temperature of the reaction mixture e. Addition of helium gas to the reaction mixture at constant volume f. Decreasing the volume of the container at constant temperature 36. In the preceding questions 2 and 3, which change(s) will alter the value of K c? Calculating Kc From Concentrations, Calculating Concentrations From Kc 37. At 460 C, the reaction has K c = A reaction flask at 460 C contains these gases at the following concentrations: [SO 2 ] = M, [NO 2 ] = M, [NO] = M, [SO 3 ] = M. a. Is the reaction at equilibrium? b. If not, which way will the reaction have to proceed to arrive at equilibrium? 38. At high temperature, 2.00 mol of HBr was placed in a 4.00 L container where it decomposed to give the equilibrium At equilibrium, the concentration of Br 2 was measured to be M. What is K c for this reaction at this temperature? 39. At 25 C, mol O 2 and mol N 2 O were placed in a 1.00 L container where the following equilibrium was then established: At equilibrium, the NO 2 concentration was M. What is the value of K c for this reaction? 40. At 25 C, K c = for the following reaction in the solvent CCl 4 :

7 If the initial concentrations of each substance in a solution are M, what will their equilibrium concentrations be? 41. The reaction 2HCl(g) H 2 (g) + Cl 2 (g) has K c = at 25 C. If a reaction vessel contains initially mol L 1 of HCl which then reacts to reach equilibrium, what will be the concentrations of H 2 and Cl 2? 42. At 2000 C, the decomposition of CO 2, has K c = If a 1.00 L container holding mol of CO 2 is heated to 2000 C, what will be the concentration of CO at equilibrium?

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