Answered: 4. Based on their activation energies…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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4. A to C

$LEARNING ACTIVITY 7 1. In which of the following reactions would you expect the orientation factor to be more important in leading to reaction: 03+0- 202 or NO+ NO. - 2NO2? Justify your answer. 2. Indicate whether each statement is TRUE or FALSE. Justify your answer. a. A reaction that has a small rate constant must have a small frequency factor. b. A smaller ratio of effectively oriented collisions to all possible collisions, would lead to a smaller orientation factor. c. Exothermic reactions are faster than endothermic reactions. d. If you compare two reactions with similar collision factors, the one with the larger activation energy will be faster. f. If you measure the rate constant for a reaction at different temperatures, you can calculate the overall enthalpy change for the reaction. g. Increasing the reaction temperature increases the fraction of successful collisions between reactants 3. For the elementary process N:Os(g) → NO:(g) + NO:(g) the activation energy and overall AE are 154 kJ/mol and 136 kJ/mol, respectively. a. Sketch the energy profile for this reaction, and label E, and AE. b. Is the reaction exothermic or endothermic? c. What is the activation energy for the reverse reaction? 4. Based on their activation energies and energy changes and assuming that all collision factors are the same, rank the REVERSE of following reactions from slowest to fastest. a. Ea- 75 kJ/mol; AE = -20 kJ/mol b. Ea- 100 kJ/mol; AE = +30 kJ/mol c. E, = 85 kJ/mol; AE = -50 kJ/mol 5. 2NO(g) - Na(g) and Oz(g) is second order with a rate constant of 0.0796 M1s' at 737 °C and 0.0815 M's at 947 °C. Calculate the activation energy for the reaction.$

Transcribed Image Text:LEARNING ACTIVITY 7 1. In which of the following reactions would you expect the orientation factor to be more important in leading to reaction: 03+0- 202 or NO+ NO. - 2NO2? Justify your answer. 2. Indicate whether each statement is TRUE or FALSE. Justify your answer. a. A reaction that has a small rate constant must have a small frequency factor. b. A smaller ratio of effectively oriented collisions to all possible collisions, would lead to a smaller orientation factor. c. Exothermic reactions are faster than endothermic reactions. d. If you compare two reactions with similar collision factors, the one with the larger activation energy will be faster. f. If you measure the rate constant for a reaction at different temperatures, you can calculate the overall enthalpy change for the reaction. g. Increasing the reaction temperature increases the fraction of successful collisions between reactants 3. For the elementary process N:Os(g) → NO:(g) + NO:(g) the activation energy and overall AE are 154 kJ/mol and 136 kJ/mol, respectively. a. Sketch the energy profile for this reaction, and label E, and AE. b. Is the reaction exothermic or endothermic? c. What is the activation energy for the reverse reaction? 4. Based on their activation energies and energy changes and assuming that all collision factors are the same, rank the REVERSE of following reactions from slowest to fastest. a. Ea- 75 kJ/mol; AE = -20 kJ/mol b. Ea- 100 kJ/mol; AE = +30 kJ/mol c. E, = 85 kJ/mol; AE = -50 kJ/mol 5. 2NO(g) - Na(g) and Oz(g) is second order with a rate constant of 0.0796 M1s' at 737 °C and 0.0815 M's at 947 °C. Calculate the activation energy for the reaction.

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