The values of the rate constant for the reaction 2 N₂O5(g) - 4 NO2(g) + O2(g) were determined at several temperatures. A plot of (In k) versus (1/T) gave a straight line of which the slope and intercept were found to be -1.2×104 and 2.32x10+¹4 respectively, calculate the activation energy of the reaction in kJ/mol? 04.0×10¹5 Ⓒ3.0*10*6 08.0×10+4 10×10¹2 O2.0*10*3

The values of the rate constant for the reaction 2 N₂O5(g) - 4 NO2(g) + O2(g) were determined at several temperatures. A plot of (In k) versus (1/T) gave a straight line of which the slope and intercept were found to be -1.2×104 and 2.32x10+¹4 respectively, calculate the activation energy of the reaction in kJ/mol? 04.0×10¹5 Ⓒ3.0106 08.0×10+4 10×10¹2 O2.0103

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 11.57PAE

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