Cblackboard.sc.eduContentBlackboard Lea...> Recitation W3... JLate Model Ca...rate = k[N₂01²Question 3Worksheet 13.6 #2XConsider the two-step mechanism below that has been proposed for the reaction of nitrous oxide to form nitrogen and oxygen gas to answer the following questiStep 1: N₂0 (g) → N2 (9) + O (g)(slow)(fast)Step 2: N₂O(g) + O (g) → N2 (g) + O2 (9)Net: 2 N₂O (g) → 2 N2 (9) + O2 (9)Part B: Based on the proposed rate law for the net overall reaction, what is the overall order of the reaction?Selected Answer:1/2 orderWorksheet 13.6 #2Consider the two-step mechanism below that has been proposed for the reaction of nitrous oxide to form nitrogen and oxygen gas to answer the following questiStep 1: N₂O (g) → N₂ (g) + O (9)(slow)(fast)Step 2: N₂O(g) + O (g) → N₂ (9) + 02 (9)Net: 2 N₂0 (g) → 2 N2 (9) + 02 (9)Part C: What intermediates/catalysts are present in this mechanism?Selected Answer:N₂O is a catalyst; there are no intermediatesWednesday, April 6, 2022 4:00:55 PM EDT80Blackboard Lea...Question 4Blackboard Lea...999F4*<MacBook AirF6&817DII

The rate of a reaction is given as the change in concentration of the reactants or the products with…

Question 3 Worksheet 13.6 #2 Consider the two-step mechanism below that has been proposed for the reaction of nitrous oxide to form nitrogen and oxygen gas to answer the following questi Step 1: N₂0 (9)→ N2 (9) + 0 (g) (slow) (fast) Step 2: N₂0 (g) + O (g) → N₂ (g) + O2(g) Net: 2 N₂0 (g) → 2 N₂ (9) + 02 (9) Part B: Based on the proposed rate law for the net overall reaction, what is the overall order of the reaction? Selected Answer: 1/2 order Worksheet 13.6 #2 X Consider the two-step mechanism below that has been proposed for the reaction of nitrous oxide to form nitrogen and oxygen gas to answer the following quest Step 1: N₂0 (g) → N₂ (g) + O(g) (slow) (fast) Step 2: N₂0 (g) + O (g) → N₂ (9) + 02 (9) Net: 2 N₂0 (g) → 2 N2 (9) + 02 (9) Part C: What intermediates/catalysts are present in this mechanism? Selected Answer: N₂O is a catalyst; there are no intermediates nesday, April 6, 2022 4:00:55 PM EDT Question 4

Question 3 Worksheet 13.6 #2 Consider the two-step mechanism below that has been proposed for the reaction of nitrous oxide to form nitrogen and oxygen gas to answer the following questi Step 1: N₂0 (9)→ N2 (9) + 0 (g) (slow) (fast) Step 2: N₂0 (g) + O (g) → N₂ (g) + O2(g) Net: 2 N₂0 (g) → 2 N₂ (9) + 02 (9) Part B: Based on the proposed rate law for the net overall reaction, what is the overall order of the reaction? Selected Answer: 1/2 order Worksheet 13.6 #2 X Consider the two-step mechanism below that has been proposed for the reaction of nitrous oxide to form nitrogen and oxygen gas to answer the following quest Step 1: N₂0 (g) → N₂ (g) + O(g) (slow) (fast) Step 2: N₂0 (g) + O (g) → N₂ (9) + 02 (9) Net: 2 N₂0 (g) → 2 N2 (9) + 02 (9) Part C: What intermediates/catalysts are present in this mechanism? Selected Answer: N₂O is a catalyst; there are no intermediates nesday, April 6, 2022 4:00:55 PM EDT Question 4

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.65PAE

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11.48 The following data were collected for the decomposition of NT),-: Time, f (min) [N2Os] (mol L-1) 0 0.200 5 0.171 10 0.146 15 0.125 20 0.106 25 0.0909 30 0.0777 35 0.0664 40 0.0570 Use appropriate graphs to determine the rate constant for this reaction. Find the half-life of the reaction.
At low temperatures, the rate law for the reaction CO(g)+NO2(g)CO2(g)+NO(g)is as follows: rate=(constant)[ NO2 ]2. Which of the following mechanisms is consistent with the rate law? (a) CO+NO2CO2+NO(b) 2NO2N2O4(fast) N2O4+2CO2CO2+2NO(slow) (c) 2NO2NO3+NO(slow) NO3+CONO2+CO2(fast) (d) 2NO22NO+O2(slow) O2+2CO2CO2(fast)
Can a reaction mechanism ever be proven correct? Can it be proven incorrect?
Regular ?ights of supersonic aircraft in the stratosphere ale of concern because such aircraft produce nitric oxide, NO, as a byproduct in the exhaust of their engines. Nitric oxide reacts with ozone, and it has been suggested that this could contribute to depletion of the ozone layer. The reaction NO+O3NO2+O2 is first order with respect to both NO and O3 with a rate constant of 2.20107 L/mol/s. What is the instantaneous rate of disappearance of NO when [NO]=3.3106 M and [O3]=5.9107M?
Some bacteria are resistant to the antibiotic penicillin because they produce penicillinase, an enzyme with a molecular weight of 3104 g/mol that converts penicillin into inactive molecules. Although the kinetics of enzyme-catalyzed reactions can be complex, at low concentrations this reaction can be described by a rate equation that is first order in the catalyst (penicillinase) and that also involves the concentration of penicillin. From the following data: 1.0 L of a solution containing 0.15 g ( 0.15106 g) of penicillinase, determine the order of the reaction with respect to penicillin and the value of the rate constant. [Penicillin] (M) Rate (mol/L/min) 2.0106 1.01010 3.0106 1.51010 4.0106 2.01010
For a certain reaction, Ea is 135 kJ and H=45 kJ. In the presence of a catalyst, the activation energy is 39% of that for the uncatalyzed reaction. Draw a diagram similar to Figure 11.14 but instead of showing two activated complexes (two humps) show only one activated complex (i.e., only one hump) for the reaction. What is the activation energy of the uncatalyzed reverse reaction?
Azomethane decomposes into nitrogen and ethane at high temperatures according to the following equation: (CH3)2N2(g)N2(g)+C2H6(g)The rate of the reaction is followed by monitoring the disappearance of the purple color due to iodine. The following data are obtained at a certain temperature. (a) By plotting the data, show that the reaction is first-order. (b) From the graph, determine k. (c) Using k, find the time (in hours) that it takes to decrease the concentration to 0.100 M. (d) Calculate the rate of the reaction when [ (CH3)2N2 ]=0.415M.
Use the data provided in a graphical method to determine the order and rate constant of the following reaction: 2PQ+W Time (s) 9.0 13.0 18.0 22.0 25.0 [P] (M) 1.077103 1.068103 1.055103 1.046103 1.039103
A proposed mechanism for the gas-phase chlorination of methane is Cl2+CH4CH4Cl+ClCH4ClCH3+HClCH3+Cl2CH3Cl+ClCl+CH4CH3+HCl Suppose the first step is the RDS. What is the expected rate law in terms of the original reactants, Cl2 and CH4? How would you determine if this mechanism might be a potentially correct or, for that matter, a potentially incorrect one?
The hypothetical reaction X(g)+12Y(g)productsis first-order in X and second-order in Y. The rate of the reaction is 0.00389 mol/L min when [X] is 0.150 M and [Y] is 0.0800 M. (a) What is the value for k? (b) At what concentration of [Y] is the rate 0.00948 mol/L min and [X] is 0.0441 M? (c) At what concentration of [X] is the rate 0.0124 mol/L min and [ Y ]=2[ X ]?
For the reaction A + B C, explain at least two ways in which the rate law could be zero order in chemical A.
Consider the following initial rate data for the decomposition of compound AB to give A and B: [AB]o (mol/L) Initial Rate (mol/L s) 0.200 3.20 103 0.400 1.28 102 0.600 2.88 102 Determine the half-life for the decomposition reaction initially having 1.00 M AB present.