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For the reaction: 2 N₂O5(g) - 4 NO2(g) + O₂(g) the rate law is: Δ[02] = At At 300 K, the half-life is 2.50 x 104 seconds and the activation energy is 103.3 kJ/mol. What is the rate constant at 310 K? O K[N₂05] O 2.78 x 10-5 S-1 7.29 x 10-6 s-1 7.29 × 10-8 S-1 3.70 x 10-5 5-1 1.05 x 10-4 s-1

For the reaction: 2 N₂O5(g) - 4 NO2(g) + O₂(g) the rate law is: Δ[02] = At At 300 K, the half-life is 2.50 x 104 seconds and the activation energy is 103.3 kJ/mol. What is the rate constant at 310 K? O K[N₂05] O 2.78 x 10-5 S-1 7.29 x 10-6 s-1 7.29 × 10-8 S-1 3.70 x 10-5 5-1 1.05 x 10-4 s-1

Chemistry
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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For the reaction: 2 N₂O5(g) - 4 NO2(g) + O₂(g) the rate law is: A[02] At O At 300 K, the half-life is 2.50 x 104 seconds and the activation energy is 103.3 kJ/mol. What is the rate constant at 310 K? O = O K[N₂05] 2.78 x 10-5 S-1 7.29 x 10-6 s-1 7.29 × 10-8 S-1 3.70 × 10-5 S-1 1.05 x 10-4 S-1
Transcribed Image Text:For the reaction: 2 N₂O5(g) - 4 NO2(g) + O₂(g) the rate law is: A[02] At O At 300 K, the half-life is 2.50 x 104 seconds and the activation energy is 103.3 kJ/mol. What is the rate constant at 310 K? O = O K[N₂05] 2.78 x 10-5 S-1 7.29 x 10-6 s-1 7.29 × 10-8 S-1 3.70 × 10-5 S-1 1.05 x 10-4 S-1
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