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, C
9H
8O
4, slowly decomposes at room temperature by reacting with water in the atmosphere to produce acetic acid, HC
2H
3O
2, and 2-hydroxybenzoic acid, C
7H
6O
3 (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).
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