[Xeno Lunar]

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
Volume of flask, L: 0.135
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]

http://misterguch.brinkster.net/molarmass.html

[Hello12]

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

[Borek]

And isnt the STP, Standard Temp and Pressure.

Plesae note, that STP is not well defined.

http://en.wikipedia.org/wiki/Standard_conditions_for_temperature_and_pressure