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#### Xeno Lunar

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« on: November 12, 2008, 12:47:20 PM »
the problem is is from a lab book, the lab is called Molar Volume of Carbon Dioxide

so far I have the following data:

mass of flask, stopper, and air, g: 107.149
mass of flask, stopper, and CO2 , g: 107.221
barometric pressure, torr: 766
barometric, atm: 1.008
temperature, C: 22
temperature, K: 295.15
density of air at T1 and P1 g/L: 1.161
mass of air, g: 0.157
mass of CO2, g: 0.229
number of moles of CO2 in flask, mol: 0.005

Volume of CO2 at STP, L: ?
molar volume of CO2 at STP, L/mol: ?

Can someone please tell me how to solve for the STP datas "?" above? I am really confused..

An addition question: how do you determine a compound or a element's molar mass? Let's take CO2 and HCl for example

thax

#### macman104

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« Reply #1 on: November 12, 2008, 12:55:36 PM »

#### Hello12

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« Reply #2 on: November 24, 2008, 01:13:46 PM »
Isn't it just a simple gas equation? V=NRT/P. And isnt the STP, Standard Temp and Pressure. If it is then just substitute the figures into the equation. So N= number of moles, R=8.31 Gas constant, Temp= 298kelvin and Pressure= 100kpa so 1.0x105pa. Also the molar gas volume of any gas at STP is 22.4dm3

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