3. Rate date were obtained for the following reaction at 25 C. What is the rate law expression and rate constantfor the reaction?2A+ B + 2CD+2EInitial Rate ofFormation of D5.0 x 104 M-min51.5 x 103 M-min5.0 x 10 M-min4.5 x 103 M-minExperimentInitial [A]Initial [B]0.20 M0.20 MInitial [C]0.10 M0.30 M0.10 M0.30 M120.10 M0.20 M0.30 M0.40 M0.20 M0.60 M

The rate law expression and the rate constant for the given reaction is to be determined using the…

Answered: 3. Rate date were obtained for the…

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 11.34PAE: 11.34 Rate data were obtained at 25°C for the following reaction. What is the rate law expression...

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Similar questions

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
Nitroglycerine is an extremely sensitive explosive. In a series of carefully controlled experiments, samples of the explosive were heated to 160 C and their first-order decomposition studied. Determine the average rate constants for each experiment using the following data: Initial [C3H5N3O9] (M) 4.88 3.52 2.29 1.81 5.33 4.05 2.95 1.72 t (s) 300 300 300 300 180 180 180 180 %Decomposed 52.0 52.9 53.2 53.9 34.6 35.9 36.0 35.4
Experiments have shown that the average frequency of chirping by a snowy tree cricket (Oecanthus fultoni) depends on temperature as shown in the table. Chirping Rate (per min) Temperature (C) 178 25.0 126 20.3 100. 17.3 What is the apparent activation energy of the process that controls the chirping? What is the rate of chirping expected at a temperature of 7.5C?
The following data have been determined for the reaction: I+OCIIO+CI 1 2 3 [I] 0.10 0.20 0.30 [OCI] 0.050 0.050 0.010 Rate(mol/L/s) 3.05104 6.20104 1.83104 Determine the rate equation and the rate constant for this reaction.
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?
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
Consider a 5.000 M solution of the hypothetical com- pound R. Its decomposition is a second-order reaction and its activation energy is 57.6 kJ/mol. At 759C, the half-life of the 5.000 M solution is 8.49 h. What is the half-life of the same solution at 700C (3 significant figures)?
For a reaction involving the decomposition of Y, the following data are obtained: (a) Determine the order of the reaction. (b) Write the rate expression for the decomposition of Y. (c) Calculate k for the experiment above.
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.
For the reaction AB+C, the following data were obtained at 30 C: [A] (M) 0.230 0.356 0.557 Rate (moI/L/s) 4.17104 9.99104 2.44103 (a) What is the order of the reaction with respect to [A], and what is the rate equation? (b) What is the rate constant?
11.64 HBr is oxidized in the following reaction: 4 HBr(g) + O2(g) —• 2 H2O(g) + 2 Br,(g) A proposed mechanism is HBr + O2 -* HOOBr (slow) HOOBr + HBr — 2 HOBr (fast) HOBr + HBr — H2O + Bn (fast) Show that this mechanism can account for the correct stoichiometry. Identify all intermediates in this mechanism. What is the molecularity of each elementary’ step? Write the rate expression for each elementary' step. Identify the rate-determining step.
The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution. NH/(aq) + NO2-(aq) — N;(g) + 2 H,O(f) INH/I (mol L1) [NO21 (mol L-1, Rate = A[NJ/At (mol L-1 s’) 0.0092 0.098 3.33 X IO"7 0.0092 0.049 1.66 X 10‘7 0.0488 0.196 3.51 X 10"6 0.0249 0.196 1.80 X 10-6 Determine the rate law for this reaction and calculate the rate constant.

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