Volume of Gases in a mixture

[ecoli]

If you had 3 different gases in a container and all three had a different number of moles of gas. Could you calculate there volume seperately? (using avagadro's V=an )? Even though there are multiple gases, the particles are assumed to not take up space, so you can calculate their volume, and then their molarity, right?

[danny8522003]

I dont see why not, just plug the numbers into [MATH]V=\frac{nRT}{P}[/MATH]

[ecoli]

because pressure and temperature isn't given. The problem is actually a gaseous equilibrium problem, but I'm only given the number of moles of the 3 gases (2 reactants and 1 product) and the volume of the container to find out Q and K, with I need the concentration, in mole/L, for.

[BhavinB]

If you assume all the particles are non-interacting, then yes you can do that. Although its useless to know the volume of one gas in a mixture. Its more useful to know its pressure...which is known as the partial pressure.

 

However, many gases interact. In this case, there is a deviation from the ideal gas rule upon mixing (which assumes a uniform gas of one type of molecule).

[ecoli]

If you assume all the particles are non-interacting, then yes you can do that. Although its useless to know the volume of one gas in a mixture. Its more useful to know its pressure...which is known as the partial pressure.

 

I just need to find out the concentrations of each gas... with the information given, I believe I can do assume this. So to find the concentration of each gas, I can just divide the given number moles of each gas and divide that by the volume of the entire container for each one. Right?

[akcapr]

any gas will occupy the same space as another at the same conditions. CO2 Ethane and Chlorine at stp will take up the same volume.

[ecoli]

any gas will occupy the same space as another at the same conditions. CO2 Ethane and Chlorine at stp will take up the same volume.

 

That's what I needed to know. Thanks