A student studies the rate at which aspirin decomposes by the reaction:
$$ \mathrm{Asp}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{Sal}+\text {
Acetic Acid } $$
She weighs out \(58.5 \mathrm{mg}\) of aspirin and dissolves it, making \(10
\mathrm{mL}\) of solution in water. She heats the solution for 5 minutes at
\(90^{\circ} \mathrm{C}\), and finds that about \(10 \%\) of the aspirin is
converted to salicylic acid and acetic acid. a. How many moles of aspirin are
in the initial solution? What is the molarity of the aspirin? MM aspirin \(=180
\mathrm{g}\) ____moles____ \(\mathbf{M}\) b. What is the rate of reaction? (See
Eq. 1 on Data page.)____ moles/L min In a similar experiment with a smaller
sample, she finds that once again about \(10 \%\) of the aspirin 0 decomposes in
5 minutes at \(100^{\circ} \mathrm{C}\). What is the order of the reaction? Why?
d. What is the rate constant for the reaction? e. In another experiment she
finds that the energy of activation \(E_{a}\) for the reaction is about \(90
\mathrm{kJ}\). How long would it take for \(10 \%\) of an aspirin sample to
decompose in a person's stomach at body temcrature, \(37^{\circ} \mathrm{C}\)
____minutes
