14- Answer the following questions based on the potential energy diagram shown here: a. Does the graph represent an endothermic or exothermic reaction? b. Label the position of the reactants, products, and activated complex. c. Determine the heat of reaction, AH, (enthalpy change) for this reaction. PE (kJ) 250 200 150 100 50

14- Answer the following questions based on the potential energy diagram shown here: a. Does the graph represent an endothermic or exothermic reaction? b. Label the position of the reactants, products, and activated complex. c. Determine the heat of reaction, AH, (enthalpy change) for this reaction. PE (kJ) 250 200 150 100 50

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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Q1. According to the "collision theory" model, why does the rate of a reaction increase when temperature increases? I. There are more collisions per second. II. The molecules are vibrating with a higher frequency. III. A greater proportion of the collisions between reactants have the required activation energy for the reaction to proceed a. I only b. II only c. III only d. I,II and III e. I and III only Q2. A reaction was found to be first order with a rate constant of3.4×10−4 s−1What percentage of the starting material would remain after 2 hours? a.8.65%b.96.0%c.90.3%d.4.00%e.99.9%Q3. The half-life of a rection was calculated at 300 seconds. What \% of starting material would remain after 900 seconds? a.25%
⦁ 4. Make your own energy diagram for an exothermic reaction that does not include a catalyst and one with a catalyst (Be sure each line is a different color or labeled). Label the axis of the diagram. Then, state what a catalyst is and how a catalyst affects the reaction rate.
The following reaction energy diagram depicts another key atmospheric reaction. Label the axes, Ea (fwd), Ea (rev). and AH rxn, and transition state, and calculate the Ea (rev). * 20H 3 78 kJ 6 72 kJ O+ H20 2 1 = Potential energy; 2 = Reaction progress; 3 = Ea (fwd); 4 = transition state; 5 = Ea (rev); 6 =AH rxn; Ea (rev) = 6 kJ 1 = Potential energy; 2 = Reaction progress; 3 = Ea (rev); 4 = transition state; 5 = Ea (fwd); 6 =AH rxn; Ea (rev) = -6 kJ 1 = Reaction progress; 2 =Potential energy ; 3 = Ea (fwd); 4 = transition state; 5 = Ea (rev); 6 =AH rxn; Ea (rev) = 6 kJ 1 = Reaction progress; 2 =Potential energy ; 3 = Ea (rev); 4 = transition state; 5 = Ea (fwd); 6 =AH rxn; Ea (rev) = -6 kJ
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14. Why does the rate of the reaction decrease over time? A. Exothermic reactions lose heat which cools the reaction which decreases the reaction rate. B. As the reaction proceeds, the concentration of the products results in fewer collisions. C. As the reaction proceeds, a decrease in the concentration of reactants results in fewer successful collisions. D. Not all molecules will react and some choose to stay in their present form. E. none of the above
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16. Use the diagram to answer these questions. 75 50 25 Products Reactants -25 Reaction progress a) Is the reaction exothermic or endothermic? b) Determine the approximate value of AE for the forward reaction. Energy (kl/mol)
16. A reaction mechanism proposes three step reactions for the overall reaction and the energy diagram shows three activated states. From the proposed mechanism and energy diagram how many reaction intermediates are expected to form?A. 3 B. none C. 1 D. 2 E. 4
QUESTION 7 Match the part of the rate law with the correct term. 2 NO(g) + Cl2(g) --> 2 NOCI(g) 2. rate 3.0 mol2*s A 3.0 mol2*s A. Y rate constant vorder of reaction with respect to NO vorder of reaction with respect to Cl2 В. 1 C. 2 overall reaction order D. 3 QUESTION 8 2.
3. The graph that best describes a catalyzed (--) and un-catalyzed (___) exothermic chemical reaction is a. b. Ep(kJ) Ep(kJ) O a b d Reaction coordinate Reaction coordinate C. d. Ep(kJ) Ep(kJ) Reaction coordinate Reaction coordinate