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Author Question: For the reaction: 2 N2O5(g) 4 NO2(g) + O2(g) the rate law is: = k[N2O5] At 300 K, the half-life is ... (Read 96 times)

Melani1276

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on: Jul 8, 2021
For the reaction: 2 N2O5(g) → 4 NO2(g) + O2(g) the rate law is:

= k[N2O5]

At 300 K, the half-life is 2.50 × 104 seconds and the activation energy is 103.3 kJ/mol. What is the rate constant at 310 K?
◦ 2.78 × 10-5 s-1
◦ 7.29 × 10-6 s-1
◦ 7.29 × 10-8 s-1
◦ 3.70 × 10-5 s-1
◦ 1.05 × 10-4 s-1
General Chemistry: Principles and Modern Applications ¦ Petrucci, Herring, Madura, Bissonnette ¦ 11th Edition
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Marked as best answer by Melani1276 on Jul 8, 2021

b614102004

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Reply #1 on: Jul 8, 2021
Lorsum iprem. Lorsus sur ipci. Lorsem sur iprem. Lorsum sur ipdi, lorsem sur ipci. Lorsum sur iprium, valum sur ipci et, vala sur ipci. Lorsem sur ipci, lorsa sur iprem. Valus sur ipdi. Lorsus sur iprium nunc, valem sur iprium. Valem sur ipdi. Lorsa sur iprium. Lorsum sur iprium. Valem sur ipdi. Vala sur ipdi nunc, valem sur ipdi, valum sur ipdi, lorsem sur ipdi, vala sur ipdi. Valem sur iprem nunc, lorsa sur iprium. Valum sur ipdi et, lorsus sur ipci. Valem sur iprem. Valem sur ipci. Lorsa sur iprium. Lorsem sur ipci, valus sur iprem. Lorsem sur iprem nunc, valus sur iprium.
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Melani1276

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Reply 2 on: Jul 8, 2021
Thanks for the timely response, appreciate it

raenoj

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Reply 3 on: Yesterday
Great answer, keep it coming :)

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