chem problem 8) For the reaction 2N2O5 (g) → 4NO2 (g) + O2 (g), the following data was collected.The integrated rate law for this reaction is: In [N2O5] = - (0.0301s') t + In [N2Os]ot (seconds)[N2O5] (M)1.24 x 10-20.92 x10-20.68 x 10-20.50 x 10-²0.37 x 10-20.28 x 10-²0.15 x 10 ²10.20.30.X40.50.70.(First order)b) What is the value of the rate constant? (

8) The given reaction is : The data collected is given below :It is given that the reaction is of first order. Thus, the integrated rate law for a first order reaction for N2O5 can be given as : lnN2O5=-kt+lnN2O50 ....eq 1Here N2O5 is the concentration after time tk is the rate constantt is the time for which the substance is decayedN2O50 is the initial concentration The integrated rate law for the given reaction is given as : lnN2O5=-0.0301 s-1t+lnN2O50 ....eq 2(b) Thus, comparing eq 1 with eq 2, we get : Rate constant (k) = 0.0301 s-1

Science

Chemistry

8) For the reaction 2N2O5 (g) → 4NO2 (g) + O2 (g), the following data was collected. The integrated rate law for this reaction is: In [N2O5] = - (0.0301s"!) t+ In [N2O5]o t (seconds) [N2Os] (M) 1.24 x 10-2 0.92 x10-2 0.68 x 10-2 0.50 x 10-2 0.37 x 10-2 0.28 x 10-² 0.15 x 102 10. 20. 30. 40. 50. 70. (First order) b) What is the value of the rate constant? (

8) For the reaction 2N2O5 (g) → 4NO2 (g) + O2 (g), the following data was collected. The integrated rate law for this reaction is: In [N2O5] = - (0.0301s"!) t+ In [N2O5]o t (seconds) [N2Os] (M) 1.24 x 10-2 0.92 x10-2 0.68 x 10-2 0.50 x 10-2 0.37 x 10-2 0.28 x 10-² 0.15 x 102 10. 20. 30. 40. 50. 70. (First order) b) What is the value of the rate constant? (

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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Question

chem problem

8) For the reaction 2N2O5 (g) → 4NO2 (g) + O2 (g), the following data was collected.
The integrated rate law for this reaction is: In [N2O5] = - (0.0301s') t + In [N2Os]o
t (seconds)
[N2O5] (M)
1.24 x 10-2
0.92 x10-2
0.68 x 10-2
0.50 x 10-²
0.37 x 10-2
0.28 x 10-²
0.15 x 10 ²
10.
20.
30.
X
40.
50.
70.
(First order)
b) What is the value of the rate constant? (

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Shop Trendy CHEM 1032Cengage S19 34 https://ng.cengage.com/static/nb/ui/evo/index.html?elSBN-9781305657571 &id-430934266&isnapshotld-10652508 s19 3.4 Cengage MInbox (112) DTAP Q Search this course L ions Use the References to access important values if needed for this question. The rate constant of the elementary reaction H2(g) +Br2(g) 2HBr(g) is k 4.45x10 L mol s at 250°C, and the reaction has an activation energy of 170 kJ mol (a) Compute the rate constant of the reaction at a temperature of 289°C L mol , 1 (b) After e (b) After equal concentrations of H, and Bry are mixed at 250o C, 6,03 10' s is required for half of them to be consumed. How long will itke to consume half of the reactants if an identical experiment is performed at 289°C? Submit Answer 3 question attempts remaining Autosaved at 9:31 AM Back 9:31 2/28
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