[taylor20343]

Hi! So I am new to this forum idea, and I am just lost on this lab I am currently working on. The lab is about the ideal gas law and I did an experiment trying to find the percentage of hydrogen peroxide in the solution. Here is the information I have gathered and have solved.
Water temp: 20 C
Barometric Pressure: 763.0 mm Hg
Initial volume of air: 50 mL
After: 195 mL
Volume of O2 collected: 145 mL
Reaction Time: 7:42
T= 293 K
P= .001 atm
V= .145 mL
n= .005

and this is where I am totally lost..

1. You are now ready to solve for actual number of moles of O2. Use R = 0.0821 L·atm/mole·K
O2=____ moles

2.Calculate the theoretical number of moles of O2 there would be if the hydrogen peroxide were 100% and not an aqueous solution.

I hope it all makes sense! Thank you in advance if you can assist me!!

[Hunter2]

First we need some ideas from you.

[Arkcon]

I'd like to welcome you, taylor20343:, to the Chemical Forums, but I'd like to remind you to  read the Forum Rules{click} You agreed to the rules when you signed up for this board, and we expect you to follow them.  Like Hunter2: said, we need to see an attempt at the problem from you.

Hi! So I am new to this forum idea, and I am just lost on this lab I am currently working on. The lab is about the ideal gas law and I did an experiment trying to find the percentage of hydrogen peroxide in the solution. Here is the information I have gathered and have solved.

So you took the measurements, and have typed the results into our forum.  That's good, we couldn't have done that for you over TCP/IP.

and this is where I am totally lost..

An now theonly thing you need is the gas laws calculation that uses the raw data you have?  Why not copy, from a text book or class notes, the formula for gas laws.  Then put in some of the results you have, that match the units of the formula, and see what you get.  There is more work to do than simply plugging in, but we'll have to try first.