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The table shows the variation of the rate constant with temperature for the first-order reaction. 2N205(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. 1.74 × 10 ·5 308. 6.61 × 10 318. 2.52 x 10 4 328. 7.59 x 10 338. 2.40 x 10 Note: Reference the Fundamental constants table for additional information. kJ mol x10

The table shows the variation of the rate constant with temperature for the first-order reaction. 2N205(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. 1.74 × 10 ·5 308. 6.61 × 10 318. 2.52 x 10 4 328. 7.59 x 10 338. 2.40 x 10 Note: Reference the Fundamental constants table for additional information. kJ mol x10

Chemistry for Engineering Students
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 11.92PAE
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The table shows the variation of the rate constant with temperature for the first-order reaction. 2N205(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. 1.74 × 10 ·5 308. 6.61 × 10 318. 2.52 x 10 4 328. 7.59 x 10 338. 2.40 x 10 Note: Reference the Fundamental constants table for additional information. kJ mol x10
Transcribed Image Text:The table shows the variation of the rate constant with temperature for the first-order reaction. 2N205(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. 1.74 × 10 ·5 308. 6.61 × 10 318. 2.52 x 10 4 328. 7.59 x 10 338. 2.40 x 10 Note: Reference the Fundamental constants table for additional information. kJ mol x10
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