Need help thx Question comp568719 1012110313140 1510QUESTION 2What is the role played by NO in the following mechanism?03 + NO → NO2 + O2NO2+ O→ NO + O2OA. spectatorOB. productreactantO D. catalystOE. intermediateQUESTION 3The OH radical reacts with itself in a disproportionation type reaction accОН + ОН – H₂O + OThis rate constant at room temperature is 2.69 x 10² M-1 s-1. If the initial cfor the reaction (in seconds)?(the answer should be entered with 3 significant figures; do not enteexamples include 1.23e-8 and 1.23e8 and -1.23e-4 and 1.23e0)QUESTION 4Which of the following changes leads to a decrease in reaction rate?OA. Increase the reactant concentration.OB.Increase the frequency of collisions.Click Save and Submit to save and submit. Click Save All Answers to save all answers.416017

Note- The given question is a multiple question, hence I solved first question according to rules of…

12 60 70 8 9 10 110 13 140 3 2 5 QUESTION 2 What is the role played by NO in the following mechanism? 03 + NO → NO2 + 02 NO2 + O→ NO + O2 OA. spectator OB. product OC reactant OD. catalyst OE intermediate 10 4 15 160 17

12 60 70 8 9 10 110 13 140 3 2 5 QUESTION 2 What is the role played by NO in the following mechanism? 03 + NO → NO2 + 02 NO2 + O→ NO + O2 OA. spectator OB. product OC reactant OD. catalyst OE intermediate 10 4 15 160 17

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

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 110CP: Consider a reaction of the type aA products, in which the rate law is found to he rate = k[A]3...

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Consider a reaction of the type aA products, in which the rate law is found to he rate = k[A]3 (termolecular reactions are improbable but possible). If the first half-tife of the reaction is found to he 40. s, what is the time for the second half-life? Hint: Using your calculus knowledge, derive the integrated rate law from the differential rate law for a tennolecular reaction: Rate=d[A]dt=k[A]3
Use the data provided to graphically determine the order and rate constant of the following reaction: SO2CI2SO2+CI2 Time(s) 0 5.00103 1.00104 1.50104 [SO2CI2] (M) 0.100 0.0896 0.0802 0.0719 Time(s) 2.50104 3.00104 4.00104 [SO2CI2] (M) 0.0577 0.0517 0.0415
There are two molecules with the formula C3H6 Propane, CH3CH = CH2, is the monomer of the polymer polypropylene, which is used for indoor-outdoor carpets. Cyclopropane is used as an anesthetic: When heated to 499 C, cyclopropane rearranges (isomerizes) and forms propane with a rate constant of 5.95104s1. What is the half-life of this reaction? What fraction of the cyclopropane remains after 0.75 h at 499 C?
. The proposed reaction mechanism is as follows:i. BrO3- (aq) + H+ (aq) à HBrO3 (aq) [Fast]ii. HBrO3 (aq) + H+ (aq) à H2BrO3+ (aq) [Medium]iii. H2BrO3+ (aq) + Br- (aq) à Br2O2 (aq) + H2O (ℓ) [Slow]iv. Br2O2 (aq) + 4H+(aq) + 4Br-(aq) à 3Br2 (ℓ) + H2O (ℓ) [Fast]Evaluate the validity of this proposed reaction. Justify your answer.
The proposed reaction mechanism is as follows:i. BrO3- (aq) + H+ (aq) = HBrO3 (aq) [Fast]ii. HBrO3 (aq) + H+ (aq) = H2BrO3+ (aq) [Medium]iii. H2BrO3+ (aq) + Br- (aq) = Br2O2 (aq) + H2O (ℓ) [Slow]iv. Br2O2 (aq) + 4H+(aq) + 4Br-(aq) = 3Br2 (ℓ) + H2O (ℓ) [Fast]Evaluate the validity of this proposed reaction. Justify your answer.
A + 2B -> C (rate constant = k1, rA = -k1[A][B]2) C -> A + 2B (rate constant = k-1, rA = k-1[C]) C + 2A -> 2D (rate constant = k2, rA = -k2[C][A]2) reaction rate constant and the rate for A of each elementary reaction are shown in the parentheses after each reaction. Calculate the overall reaction rate for A in terms of [A], [B], k1, k-1, and k2 assuming c is psuedo-state-concentration overall chemical rxn is 3A+2B->2D
19. Predict the relative rates of these reactions. That is, select 1 next to the reaction with the fastest rate, 2 next to the reaction with the next fastest rate, and so onNote for advanced students: you may assume these reactions all take place in a polar aprotic solvent, like DMSO.
2A + B --> 3C + 2D The rate of formation of C in the above reaction is measured at 2.2 mol dm-3 s-1. What are the rates of formation and consumption of D, A, and B? Ans: 1.5 mol dm-3 s-1, 1.5 mol dm-3 s-1, and 0.73 mol dm-3 s-1 respectively.
As described in Problem P17D.5, reaction with the hydroxyl radical OH is the main path by which CH4 is removed from the lower atmosphere. T. Gierczak et al. (J. Phys. Chem. A 101, 3125 (1997)) measured the rate constants for the bimolecular gas-phase reaction CH4 + OH → CH3 + H2O and found A = 1.13 × 109 dm3 mol−1 s−1 and Ea = 14.1 kJ mol−1 for the Arrhenius parameters. (a) Estimate the rate of consumption of CH4 under the following conditions: take the average OH concentration to be 3.5 × 10−15 mol dm−3, that of CH4 to be 40 nmol dm−3, and the temperature to be −10 °C. (b) Estimate the global annual mass of CH4 consumed by this reaction (which is slightly less than the mass introduced to the atmosphere) given an effective volume for the Earth’s lower atmosphere of 4 × 1021 dm3.
17. Which of these statement is (are) true? If a statement is false, reword it so it become true. a. The concentration of homogenous catalyst may appear in the rate law. b. A catalyst is always consumed in the reactionn. 19. Why ae hoogenus catalysts harder to separate from products and leftover reactants than are heterogenous reactants? 23. The rate constant for decomposition of azomethane at 425°C is 0.68-1. CH3N=NCH3(g) ---> N2(g) + C2H6(g) a. Based on the units of the rate constant, is the reaction zeroth-, first-, or second order? b. If 2.0 g azomethane is placed in a 2.0-L flask and heated to 425°C, what mass of azomethane remains after 5.0 s? c. How long does it take for the mass of azomethane to drop to 0.24 g? d. What mass of nitrogen would be found in the flask after 0.50 s of reaction?
The reaction 2NO(g) + Cl2(g) ---> 2NOCl(g) was performed and the following data obtained: Is the following mechanism consistent with the data? Explain. NO(g) + Cl2(g) -->NOCl2(g) NOCl2(g) + NO(g) --->2NOCl(g)
What is the rate law for this elementary reaction?2NO2 ⇌ N2O4A. rate = k[NO2]2B. rate = k[NO2]xC. rate = [N2O4]/[NO2]2D. rate = k[NO2]x[N2O4]yE. rate = k[NO2]2[N2O4]