The following data were obtained for the reaction 2A → B:Time, minTA], mol/L 0.0962 0.0398 0.015610204060800.0059 0.000428 0.000061 0.000009(i)By plotting a suitable graph, determine the order of this reaction.(i)Calculate the rate constant of the reaction.

The order of the reaction can be determined by the graphical method also. there are different…

Answered: The following data were obtained for…

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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[4] Consider the following mechanism for the reaction of nitric oxide and hydrogen: kı 2NO(g)+ H2(g) → N;O(g) + H¿O(g) slow k2 N,0(g) + H2(g) → N2(g) + H2O(g) fast (a) Write an equation for the overall reaction. (b) Write the theoretical rate law for the above mechanism. (c) Is a catalyst involved in the above mechanism? If so, what is it? (d) Are there any reaction intermediates? If so, list them.
5. You studied the chemical reaction, 2NO2(g) → 2NO(g) + O2(g), at 25°C by monitoring the concentration of NO2(g) as a function of time and constructed the following graph. y= 0.5408x + 125.0 R2=0.998 Time (s) What is the rate constant for this reaction at 25°C? Include the proper units. (W/T) [(3)ONI/T
5
A reaction has a rate law of Rate = (1.25 M⁻¹s⁻¹)[A][B]. What is the rate of the reaction if [A] = 0.313 M and [B] = 0.280 M?
Which of the following is true for the rate law r= k[A]M[B]"? O A) The order of each species must be determined by experiment. B) Both m and n are restricted to positive integers. C) Both m and n can be obtained from the stoichiometry of the overall reaction. D) The overall order of the reaction is given by m x n.
Given the information based on time and concentration, determine the order of the reaction and the rate constant k when graphing the following data: A--> C+D Time (s) (A] M 10 0.1000 50 0.0856 100 0.0749 200 0.0598 350 0.0460 500 0.0373 800 0,0271
2 YO2 (g) + X2 (g) → 2 YO₂X (g) = -218 kJ/mol reaction AH rxn The reaction is first-order with respect to YO2 and first-order with respect to X₂. What is the relationship between the rate constant and activation energy of a chemical reaction?|
For the first-order reaction N2O5( g) 2 NO2 g) + → t1/2= 20.5 h at 20°C and 3.5h at 40°C. (a) Calculate the activation energy of this reaction. (b) If the Arrhenius constant A = 2.5 x 105 s', determine the value of k at 50°C.
The half-life of a reaction, t/2. is the time it takes for the reactant concentration A| to decrease by half. For example, after one half-life the concentration falls from the initial concentration [Alo to [Alo/2, after a second half-life to [A]o/4, after a third half-life to [Alo/8. and so on. on.

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The following data were obtained for the reaction 2A B: Time, min [A], mol/L| 0.0962 10 0.0156 40 0.0059 0.000428 0.000061 | 0.000009 20 60 80 | 0.0398 (1) By plotting a suitable graph, determine the order of this reaction. (ii) Calculate the rate constant of the reaction.