## 15.11

$aR \to bP, Rate = -\frac{1}{a} \frac{d[R]}{dt} = \frac{1}{b}\frac{d[P]}{dt}$

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### 15.11

N2O5 decomposes by a first-order run. Whats the initial rate of decamp when 3.45g is confined in 0.75L container and heated to 65C? k=5.2E-3.

I understand the answer, but was wondering if we should just ignore the temp?

Thanks!

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### Re: 15.11

Yes, for this question I simply ignored the temperature, because I think the only reason it was given is just to give context as to why it's a decomposition reaction. Since it's a first order reaction, the rate will be k * [A]. We are given k, but have to solve for concentration using the given grams of N2O5 as well as its molar mass. Then, all we do is simply plug in these values to obtain the rate of 2.2 x 10^(-4) mol/(L*s).