(adsbygoogle = window.adsbygoogle || []).push({}); 1. The problem statement, all variables and given/known data

The air in a bicycle tire is bubbled through water and collected at 25 [tex]^\circ {\rm C}[/tex]. If the total volume of gas collected is 5.25 L at a temperature of 25 [tex]^\circ {\rm C}[/tex] and a pressure of 734 torr, how many moles of gas was in the bicycle tire?

2. Relevant equations

PV = nRT

[tex]n=\frac{PV}{RT}[/tex]

R = .08206

3. The attempt at a solution

1. Convert 734 torr to atm

734/760 = .966 atm

2. Convert 25 [tex]^\circ {\rm C}[/tex] to K = 298.15 K

3. Plug those all in:

[tex]n=\frac{(.966 atn)(5.25 L)}{(.08206)(298.15 K)}[/tex]

I got n=.207 moles, but the online assignment says I got it wrong.

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# Homework Help: CHEMISTRY: Partial Pressure

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