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blue powder
Registered User regular

Just to clarify, this is a question I'm doing from a past exam paper in preparation for an up coming exam. So I'm not asking you guys to do my homework haha.

The question is: "What is the average distance between argon atoms in a sample of argon gas at standard temperature and pressure (STP = 0C and 1 atm)?" At the STP, the molar volume of an ideal gas is 22.4 L. The atomic mass of argon is 40.0 amu.

So from this my working out is as follows:

22.4L/40amu = 0.56 * 6.02x10^23

= (i'm not sure how to get that cubed divide sign up-ask me if you don't know what i mean, sorry!) 3.37x10^23

= 69597692.26

= 1/69597692.26

= 1.43x10^-8 m

I'm not sure I have my units correct... This is just a weird way for me to approach a question like that as I'm used to doing it with a solid and using the density. Thanks in advance!

The question is: "What is the average distance between argon atoms in a sample of argon gas at standard temperature and pressure (STP = 0C and 1 atm)?" At the STP, the molar volume of an ideal gas is 22.4 L. The atomic mass of argon is 40.0 amu.

So from this my working out is as follows:

22.4L/40amu = 0.56 * 6.02x10^23

= (i'm not sure how to get that cubed divide sign up-ask me if you don't know what i mean, sorry!) 3.37x10^23

= 69597692.26

= 1/69597692.26

= 1.43x10^-8 m

I'm not sure I have my units correct... This is just a weird way for me to approach a question like that as I'm used to doing it with a solid and using the density. Thanks in advance!

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## Posts

Al_waton69597692.26 should be 6.96 * 10^7. Makes them a lot easier to deal with because the exactness of the numbers you round are almost never necessary.

VeritasVRonLet 'em eat fucking pineapples!Also, it seems ok. I never liked that particular problem, however.

Iceman.USAFonPeekingDuckonDemerdaronI got an A in a level chemistry simply by always using units (plus a load of pointless memorising, but you don't need so much of that for physics).

corcoriganon