CHAPTER 17 REVIEW. Reaction Kinetics. Answer the following questions in the space provided. Energy B A. Course of reaction
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1 CHAPTER 17 REVIEW Reaction Kinetics SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. Refer to the energy diagram below to answer the following questions. D Energy C d c d c b B A Course of reaction a. Which letter represents the energy of the activated complex? (a) A (c) C (b) B (d) D b. Which letter represents the energy of the reactants? (a) A (c) C (b) B (d) D c. Which of the following represents the quantity of activation energy for the forward reaction? (a) the amount of energy at C minus the amount of energy at B (b) the amount of energy at D minus the amount of energy at A (c) the amount of energy at D minus the amount of energy at B (d) the amount of energy at D minus the amount of energy at C d. Which of the following represents the quantity of activation energy for the reverse reaction? (a) the amount of energy at C minus the amount of energy at B (b) the amount of energy at D minus the amount of energy at A (c) the amount of energy at D minus the amount of energy at B (d) the amount of energy at D minus the amount of energy at C e. Which of the following represents the energy change for the forward reaction? (a) the amount of energy at C minus the amount of energy at B (b) the amount of energy at B minus the amount of energy at C (c) the amount of energy at D minus the amount of energy at B (d) the amount of energy at B minus the amount of energy at A MODERN CHEMISTRY REACTION KINETICS 137
2 SECTION 1 continued 2. For the reaction described by the equation A B X, the activation energy for the forward direction equals 85 kj/mol and the activation energy for the reverse direction equals 80 kj/mol. the product 5 kj/mol True a. Which has the greater energy content, the reactants or the product? b. What is the enthalpy of reaction in the forward direction? c. The enthalpy of reaction in the reverse direction is equal in magnitude but opposite in sign to the enthalpy of reaction in the forward direction. True or False? 3. Below is an incomplete energy diagram. Activated Complex Energy (kj/mol) 50 E a Reactants E 10 E á 60 Products Forward Reverse a. Use the following data to complete the diagram: E a 50 kj/mol; E forward 10 kj/mol. Label the reactants, products, E, E a, E a, and the activated complex. 60 kj/mol b. What is the value of E a? 4. It is proposed that ozone undergoes the following two-step mechanism in our upper atmosphere. O 3 (g) O 2 (g) O(g) O 3 (g) O(g) 2O 2 (g) a. Identify any intermediates formed in the above equations. Monatomic O is the intermediate formed. b. Write the net equation. 2O 3 (g) 3O 2 (g) exothermic c. If E is negative for the reaction in part b, what type of reaction is represented? 138 REACTION KINETICS MODERN CHEMISTRY
3 CHAPTER 17 REVIEW Reaction Kinetics SECTION 2 SHORT ANSWER Answer the following questions in the space provided. 1. Below is an energy diagram for a particular process. One curve represents the energy profile for the uncatalyzed reaction, and the other curve represents the energy profile for the catalyzed reaction. 1 Energy (kj/mol) 2 Course of reaction a a. Which curve has the greater activation energy? (a) curve 1 (b) curve 2 (c) Both are equal. c b. Which curve has the greater energy change, E? (a) curve 1 (b) curve 2 (c) Both are equal. b c. Which curve represents the catalyzed process? (a) curve 1 (b) curve 2 d. Explain your answer to part c. The catalyst forms an alternative activated complex that requires a lower activation energy, as represented by the lower curve. MODERN CHEMISTRY REACTION KINETICS 139
4 SECTION 2 continued 2. Is it correct to say that a catalyst affects the speed of a reaction but does not take part in the reaction? Explain your answer. It is not correct. The catalyst does take part in the reaction. However, if it is used up in one step of the mechanism, it is regenerated in a later step. There is no net change in mass for the catalyst. 3. The reaction described by the equation X Y Z is shown to have the following rate law: R k[x] 3 [Y] a. What is the effect on the rate if the concentration of Y is reduced by one-third and [X] remains constant? The rate is reduced by one-third as well. b. What is the effect on the rate if the concentration of X is doubled and [Y] remains constant? The rate increases by a factor of eight. c. What is the effect on the rate if a catalyst is added to the system? The rate will increase if the catalyst added is specific for this reaction. 4. Explain the following statements, using collision theory: a. Gaseous reactants react faster under high pressure than under low pressure. At high pressure, gas molecules are more closely packed and collide more frequently. Thus, more-effective collisions occur per unit of time. b. Ionic compounds react faster when in solution than as solids. Ions in solution have more freedom of motion than do ions in a solid; therefore, they can collide with one another more frequently. c. A class of heterogeneous catalysts called surface catalysts work best as a fine powder. The fine powder has more surface area on which reactant particles can be absorbed and, in effect, increases the concentration of the reactants. An increase in concentration increases the number of effective collisions between reactant particles. 140 REACTION KINETICS MODERN CHEMISTRY
5 CHAPTER 17 REVIEW Reaction Kinetics MIXED REVIEW SHORT ANSWER Answer the following questions in the space provided. 1. The reaction for the decomposition of hydrogen peroxide is 2H 2 O 2 (aq) 2H 2 O(l) O 2 (g). List three ways to speed up the rate of decomposition. For each one, briefly explain why it is effective, based on collision theory. increase the concentration of hydrogen peroxide allows more collisions per unit of time to occur increase the temperature of the solution allows more energetic collisions per unit of time to occur stir the solution exposes more reactant surface area, which allows more collisions per unit of time to occur add a catalyst lowers the activation energy so that more-effective collisions can occur 2. An ingredient in smog is the gas NO. One reaction that controls the concentration of NO is H 2 (g) 2NO(g) H 2 O(g) N 2 O(g). At high temperatures, doubling the concentration of H 2 doubles the rate of reaction, while doubling the concentration of NO increases the rate fourfold. Write a rate law for this reaction consistent with these data. R k[h 2 ][NO] 2 3. Use the following chemical equation to answer the question below: Mg(s) 2H 3 O (aq) Cl (aq) Mg 2 (aq) 2Cl (aq) H 2 (g) H 2 O(l) If g of magnesium completely reacts in 20 s, what is the average reaction rate in moles/second over that time interval? Average rate mol/s MODERN CHEMISTRY REACTION KINETICS 141
6 MIXED REVIEW continued PROBLEMS provided. Write the answer on the line to the left. Show all your work in the space 4. Answer the following questions using the energy diagram below Energy (kj/mol) Course of reaction endothermic 40 kj/mol a. Is the forward reaction represented by the curve exothermic or endothermic? b. Estimate the magnitude and sign of E forward. 20 kj/mol c. Estimate E a. A catalyst is added to the reaction, which lowers E a by about 15 kj/mol. speed up d. Does the forward reaction rate speed up or slow down? speed up e. Does the reverse reaction rate speed up or slow down? No f. Does E forward change from its value in part b? 5. a. Determine the overall balanced equation for a reaction having the following proposed mechanism: Step 1: 2NO H 2 N 2 H 2 O 2 Slow Step 2: H 2 H 2 O 2 2H 2 O Fast 2NO 2H 2 N 2 2H 2 O b. Which is the rate-determining step? Step 1 c. What is the intermediate in the above reaction? H 2 O REACTION KINETICS MODERN CHEMISTRY
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