We are being asked to determine the partial pressure of O_{2} given the following first-order reaction:

N_{2} O_{5(g)}→ NO_{2(g) }+ O_{2(g) }; **k = 1.0x10**^{ - 5 }**hr**^{- 1}

For this problem, we will do the following steps:

**Step 1: Calculate [A****] at time t using the first-order integrated rate law**

The ** integrated rate law** for a first-order reaction is as follows:

$\overline{){\mathbf{ln}}{\left[\mathbf{A}\right]}_{{\mathbf{t}}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{\mathbf{-}}{\mathbf{kt}}{\mathbf{}}{\mathbf{+}}{\mathbf{}}{\mathbf{ln}}{\left[\mathbf{A}\right]}_{{\mathbf{0}}}}$

where **[A] _{t}** = concentration at time t,

Dinitrogen pentoxide (N_{2} O_{5}) decomposes in chloroform as a solvent to yield NO_{2} and O_{2}. The decomposition is first order with a rate constant at 45 ^{o}C of 1.0x10^{ - 5 }hr^{- 1}.

Calculate the partial pressure of O_{2} produced from 1.51 L of 0.601 M N_{2} O_{5} solution at 45 ^{o}C over a period of 20.1 h if the gas is collected in a 11.6-L container. (Assume that the products do not dissolve in chloroform.)

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Based on our data, we think this problem is relevant for Professor Chilom's class at DIXIE.