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Mass density of a gas!

by warrior2014
Tags: density, mass
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warrior2014
#1
Nov28-11, 08:42 PM
P: 34
1. The problem statement, all variables and given/known data
At 0 degrees, and 1 atm, 0.6 mol of a gas occupies a volume of 0.0134 m^3. what is the mass density? The number density is 2.69x10^25 m-3, the average distance between the gas molecule is 4nm and the total mass is 17.685g.


2. Relevant equations

n=N/Na

1u=1.66x10^-27 mol-1

3. The attempt at a solution

I tried to find N so I did 0.6/6,022x10^23 and got 9.96x10^-25. Then I multiplied this by 2.69x 10^-25 and go 2.68x10^-49 which was wrong.

I'm not exactly sure how to solve the problem, so any help is appreciated!
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cepheid
#2
Nov28-11, 08:52 PM
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Quote Quote by warrior2014 View Post
1. The problem statement, all variables and given/known data
At 0 degrees, and 1 atm, 0.6 mol of a gas occupies a volume of 0.0134 m^3. what is the mass density? The number density is 2.69x10^25 m-3, the average distance between the gas molecule is 4nm and the total mass is 17.685g.
I'm confused. You have the total mass, and you have the volume it occupies. So, what is stopping you from computing the mass density from that information alone?

Quote Quote by warrior2014 View Post
2. Relevant equations

n=N/Na

1u=1.66x10^-27 mol-1

3. The attempt at a solution

I tried to find N so I did 0.6/6,022x10^23 and got 9.96x10^-25. Then I multiplied this by 2.69x 10^-25 and go 2.68x10^-49 which was wrong.

I'm not exactly sure how to solve the problem, so any help is appreciated!
As an aside, the step in red above is wrong. It should be (0.6 mol)*(6.022x1023
molecules/mol), which you can see gives you a result in "molecules." Always include units in calculations like this in order to catch errors like this.


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