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Author Question: Aspirin, C9H8O4, slowly decomposes at room temperature by reacting with water in the atmosphere to ... (Read 36 times)

jlol3

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on: Nov 5, 2023

Question 1

An experimental drug, D, is known to decompose in the blood stream. Tripling the concentration of the drug increases the decomposition rate by a factor of nine. Write the rate law for decomposition of D and give the units of the rate constant.

Question 2

Aspirin, C9H8O4, slowly decomposes at room temperature by reacting with water in the atmosphere to produce acetic acid, HC2H3O2, and 2-hydroxybenzoic acid, C7H6O3 (this is why old bottles of aspirin often smell like vinegar):
         
C9H8O4 + H2O → HC2H3O2 + C7H6O3
         
         Concentration and rate data for this reaction are given below.
[C9H8O4] (M)
[H2O] (M)
Rate (M/s)
   0.0100
 0.0200
2.4 × 10–13
   0.0100
 0.0800
9.6 × 10–13
   0.0200
 0.0200
4.8 × 10–13
         
Write the rate law for this reaction and calculate k (be sure to include the correct units).
Chemistry ¦ Chang, Goldsby ¦ 11th Edition
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Marked as best answer by jlol3 on Nov 5, 2023

ElaneShive

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Reply #1 on: Nov 5, 2023
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jlol3

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Reply 2 on: Nov 5, 2023
:D TYSM

xoxo123

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Reply 3 on: Yesterday
Wow, this really help

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