The table shows the variation of the rate constant with temperature for the first-order reaction. 2N₂O(g) 2N₂O4(g) + O₂(g) Determine graphically the activation energy for the reaction. Round your answer to 2 significant digits. |T (K) | K (¹) 298. 308. 318. 328. 338. 1.74 x 105 6.61 x 105 2.52 x 10 7.59 x 104 2.40 × 10-3 Note: Reference the Fundamental constants table for additional information. kJ mol S

The table shows the variation of the rate constant with temperature for the first-order reaction. 2N₂O(g) 2N₂O4(g) + O₂(g) Determine graphically the activation energy for the reaction. Round your answer to 2 significant digits. |T (K) | K (¹) 298. 308. 318. 328. 338. 1.74 x 105 6.61 x 105 2.52 x 10 7.59 x 104 2.40 × 10-3 Note: Reference the Fundamental constants table for additional information. kJ mol S

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

#45

45
The table shows the variation of the rate constant with temperature for the first-order reaction.
2N₂O5 (g)
2N₂O4(g) + O₂(g)
Determine graphically the activation energy for the reaction. Round your answer to 2 significant digits.
* (+/-)
S
T (K) k
298.
308.
1.74 × 10
328.
6.61 × 10
318. 2.52 × 10
7.59 × 10
338. 2.40 × 10
-5
kJ
mol
-5
-4
-4
3
Note: Reference the Fundamental constants table for additional information.
x10
X
5

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