6. (0,5 points) One method for the destruction of ozone in the upper atmosphere is: O3 NO NO, + O2 (slow) NO2 NO O2 (fast) + O3 202 + Overall reaction: Task Answer Which species is an intermediate? Which species is a catalyst? Which is the rate-determining step? Number of times each reactant is used in the rate- determining step? Write the ratelaw for the reaction.

6. (0,5 points) One method for the destruction of ozone in the upper atmosphere is: O3 NO NO, + O2 (slow) NO2 NO O2 (fast) + O3 202 + Overall reaction: Task Answer Which species is an intermediate? Which species is a catalyst? Which is the rate-determining step? Number of times each reactant is used in the rate- determining step? Write the ratelaw for the reaction.

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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3.2. What is the expression for the rate of appearance of NO based upon the following reaction? 2 NOCI(g) Cl₂(g) + 2NO(g) a. rateNocl c. rateNocl = 2 == 1 A[NO] 2 At A[NO] At a 1.3 x 10-³ M/s b. 1.9 x 10-3 M/s c. 2.5 x 10-3 M/s d. 5.0 x 10-3 M/s b. d. rate NOCI rate NOCI = = A[NO] At A[NO] At What is the numerical value for the rate of reaction if the rate of disappearance of NOCI is 5.0 x 10-3 M/s?
Hydrogen gas reduces NO to N2 in the following reaction:$$2H2(g)+2NO(g)2H2O(g)+N2(g)The initial reaction rates of four mixtures of H2 and NO were measured at 1500°C with the following results: Experiment [H2]0 (M) [NO]0 (M) Initial Rate (M/s) 1 0.212 0.136 0.0387 2 0.212 0.272 0.0777 3 0.424 0.544 0.615 4 0.848 0.544 2.47 Determine the rate constant for the reaction at 1500°C. M-xs-1
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4. 13.67 5. The following diagrams represent the progress of the reaction AB, where the red spheres represent A molecules and the green spheres represent B mole- cules. Calculate the rate constant of the reaction. 1=0 s 1 = 20 s t = 40 s
(14.37] Consider the gas-phase reaction batween nitric axide and bromine at 273 "C: 2 NO() + Brfg) 3 NOBr(g). The following data for the initial rate of appearance of NOBT were obtained: as Experiment [NO] (M) [Br (M) Initial Rate (M/s) 0.10 0.20 24 0.25 0.20 150 0.10 0,50 60 0.35 0.50 795 (a) Determine the rate hw. (b) Calcalate the average valueof the rate constant tor the appearance of NOET from the four data sets. (c) How is the rate of appearance of NOBr related to the rate of disappearance of Bri (d) What is the rate of disap- pearance of Br2 when (NO) 0.075 M and (Bra) 0.25 M?
Hydrogen gas reduces NO to N2 in the following reaction:$$2H2(g)+2NO(g)2H2O(g)+N2(g)The initial reaction rates of four mixtures of H2 and NO were measured at 1500°C with the following results: Experiment [H2]0 (M) [NO]0 (M) Initial Rate (M/s) 1 0.212 0.136 0.0333 2 0.212 0.272 0.0669 3 0.424 0.544 0.528 4 0.848 0.544 2.12 Determine the rate constant for the reaction at 1500°C.
For the reaction 2NO + 2H2 → N2 + 2H2O, the rate equation is rate = k[NO]2[H2]. The overall order of the reaction is ____. Select one: A. 2 B. 4 C. 3 D. 1
9:50 PM Mon Feb 13 The reaction A + 2B → C has the rate law rate= K[A] [B]. By what factor does the rate of reaction increase when both [A] and [B] are doubled? Tap here or pull up for additional resources 1 2 #3 $ % 5 Question 3 of 14 6 & 7 1 4 7 +/- ) 0
3. (14.24 Brown) For each of the following gas-phase reactions, write the rate expression in term of the appearance of each product and the disappearance of each reactant: a. 2 H₂O(g) → 2H2(g) + O2(g) b. 2SO2(g) + O2(g) → 2 SO3(g) c. 2NO(g) + 2 H2(g) → N2(g) + 2 H2O(g) d. N2(g) + 2H2(g) → N₂H4(g)
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QUESTION 2 The following mechanism has been proposed for the gas-phase exothermic reaction of chloroform (CHCl3) and chlorine: Step 1: Step 2: Step 3: Q 2(a) Cl₂2Cl Cl + CHCl3 → HCl+ CCl3 Cl + CCl3 → CCl4 i. What is the overall reaction? (fast) (slow) (fast) ii. What are the intermediates in the mechanism? iii. What is the molecularity of the elementary reactions? iv. Write down the rate law for each elementary reaction. v. What is the rate-determining step? Q 2(b) Using the rate-determining step and pre-equilibria determine the rate law predicted by this mechanism. Q2(c) Roughly sketch and label a reaction profile graph (potential energy vs reaction coordinate) for this reaction. ii. Include in the graph: reactants, products, intermediary/intermediaries, activation energy for each elementary step. iii. Compare the activation energy for all the elementary step, indicating which one is the highest.
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