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Topic: Partial Pressure Calculation  (Read 18668 times)

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Offline laxplayer

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Partial Pressure Calculation
« on: November 07, 2007, 06:15:54 PM »
The problem states:
A mixture of gases contains 5.84 g of N2, 5.31 g of H2, and 8.21 g of NH3. If the total pressure of the mixture is 2.86 atm, what is the partial pressure of each component?

I know that all of the pressures have to add up to 2.86 atm because of Dalton's Law, but that's about it :] I don't understand how you go from grams of a substance to finding pressure of it, without knowing the temperature or volume.

Online Borek

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Re: Partial Pressure Calculation
« Reply #1 on: November 07, 2007, 06:34:08 PM »
Do you know what mole fraction is and how it is related to partial pressure?
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Offline laxplayer

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Re: Partial Pressure Calculation
« Reply #2 on: November 07, 2007, 06:59:39 PM »
Aren't the mole fractions the moles of one substance over the moles of the total? But I don't know how they're related.

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Re: Partial Pressure Calculation
« Reply #3 on: November 07, 2007, 07:09:51 PM »
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Offline laxplayer

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Re: Partial Pressure Calculation
« Reply #4 on: November 07, 2007, 08:20:31 PM »
oh, so they're equal. P1/P=n1/n right? So does that mean (.2084 mol N2)/(3.32433 mol total)=(X atm N2)/(2.86 atm total)?

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Re: Partial Pressure Calculation
« Reply #5 on: November 07, 2007, 08:45:58 PM »
It says I got it right!  ;D

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