Chemistry Help

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thread starter SwiftTricky Feb 21 2010 + PM | QUOTE | PERMALINK | REPORT

A tank contains a mixture of 3.0 mol N2, 2.0 mol O2, and 1.0mol CO2 at 25degrees Celsius and a total pressure of 10.0atm. Calculate the partial pressure (in torr) of each gas in the mixure. A sample of oxygen gas is saturated with water vapor at 27degrees Celsius. The total pressure of the mixture is 772torr, and the vapor pressure of water is 26.7torr at 27degrees Celsius. What is the partial pressure of the oxygen gas? Im using the PV=nRT formula but its really hard since they dont give you volume to help calculate... 22.4L = 1mol, 760torr = 1atm Can you guys help me and explain the steps?

iBBi 02/21/10 + PM | QUOTE | PERMALINK | REPORT

What I do usually is youtube what I am learning in Chemistry. It really helps!

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SwiftTricky 02/21/10 + PM | QUOTE | PERMALINK | REPORT

Lol but its not the actual problem x-x

aznremix94 + PM | QUOTE | PERMALINK | REPORT

number 2 is confusing. o.0 edit: since your not at stp, its 25 c then you dont use 22.4 liter. pv=nrt is the ideal gas law, which you dont need to use. use p/t=p/vt, v/t=v/t or pv=pv.

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Logic 02/21/10 + PM | QUOTE | PERMALINK | REPORT

[quote] SwiftTricky : A tank contains a mixture of 3.0 mol N2, 2.0 mol O2, and 1.0mol CO2 at 25degrees Celsius and a total pressure of 10.0atm. Calculate the partial pressure (in torr) of each gas in the mixure. A sample of oxygen gas is saturated with water vapor at 27degrees Celsius. The total pressure of the mixture is 772torr, and the vapor pressure of water is 26.7too at 27degrees Celsius. What is the partial pressure of the oxygen gas? Im using the PV=nRT formula but its really hard since they dont give you volume to help calculate... 22.4L = 1mol, 760torr = 1atm Can you guys help me and explain the steps? [/quote] 1. Use Pv = nRT to solve for each pressure in atm, then convert over to torr. Knowing Dalton's law of partial pressure, total pressure in the container is equal to the partial pressures of each gas added up. 2. Total pressure of the mixture - mixture of the water = pressure of the oxygen gas. 772-26.7 = pressure of O2

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jens4life + PM | QUOTE | PERMALINK | REPORT

for the first one, use pvnert and combined moles to solve for your volume, and then solve for individual pressures.

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Logic 02/21/10 + PM | QUOTE | PERMALINK | REPORT

[quote] jens4life : for the first one, use pvnert and combined moles to solve for your volume, and then solve for individual pressures. [/quote] Or this : Partial Pressure = Total Pressure x Xa (Mol fraction : (mol of gas A / total moles) )

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SwiftTricky 02/21/10 + PM | QUOTE | PERMALINK | REPORT

cant use Pv=NRT without volume or partial gas, combining the volume will end up being 134.4L and if you have that volume and use it in P=nRT/V, you would still end up with the wrong partial pressure since ti doesnt add up to 10.0atm