Consider the following second-order decomposition reaction: N₂O5(g) → N₂O4(g) + ½ O2(g) At 318 K, it took 129.0 seconds for 50% of 12.5 M of the reactant to decompose. What is the rate constant for this reaction at this temperature? 1.03 x 10¹ M¹s1 9.69 x 10-2 M-¹-1 O 6.20 x 10-4 M¯¹s¯¹ O 2.45 x 10-3 M¯¹s-1

Consider the following second-order decomposition reaction: N₂O5(g) → N₂O4(g) + ½ O2(g) At 318 K, it took 129.0 seconds for 50% of 12.5 M of the reactant to decompose. What is the rate constant for this reaction at this temperature? 1.03 x 10¹ M¹s1 9.69 x 10-2 M-¹-1 O 6.20 x 10-4 M¯¹s¯¹ O 2.45 x 10-3 M¯¹s-1

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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