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Author Question: The oxidation of iodide ions by arsenic acid in acidic aqueous solution occurs according to the net ... (Read 62 times)

hannahmadyronde

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on: Nov 5, 2023

Question 1

Nitrogen pentoxide decomposes by a first-order process yielding N2O4 and oxygen.
         2N2O5→ 2N2O4 + O2
At a given temperature, the half-life of N2O5 is 0.90 hr.  What is the first-order rate constant for N2O5 decomposition?

Question 2

The oxidation of iodide ions by arsenic acid in acidic aqueous solution occurs according to the net reaction H3AsO4 + 3I– + 2 H3O +→ H3AsO3 + I3– + H2O. The experimental rate law for this reaction is
         Rate = k [H3AsO4] [I–] [H3O+].
According to the rate law for the reaction, an increase in the concentration of hydronium ion has what effect on this reaction?
Chemistry ¦ Chang, Goldsby ¦ 11th Edition
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Marked as best answer by hannahmadyronde on Nov 5, 2023

butterfly17

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Reply #1 on: Nov 5, 2023
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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hannahmadyronde

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Reply 2 on: Nov 5, 2023
Thanks for the timely response, appreciate it

DylanD1323

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Reply 3 on: Yesterday
Excellent

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