- #1

needphyshelp

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## Homework Statement

Hydrogen peroxide undergoes a first-order decomposition to water and O2 in aqueous solution. The rate constant at 25°C is 7.40e

^{-4}s. Calculate the volume of O2 obtained from the decomposition reaction of 1.00 mol H2O2 at 25°C and 740 mmHg after 12.4 min.

## Homework Equations

ln[H

_{2}O

_{2}]= -kt + ln[H

_{2}O

_{2}]

_{0}

## The Attempt at a Solution

12.4 minutes = 744s

k = 7.4e-2

I started using the above equation to calculate the concentration of H2O2 and then tried to get O2 from there, but that just gave me molarity and I'm not sure how to find volume. Also, the equation does not include the pressure, so I am not sure if I am using the correct equation, but I can't find anything else in the book.

Thanks :-)