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posted by  babujoo on 10/24/2008 8:05:56 AM  |  status: Live  

chemistry question

Course Textbook Chapter Problem
General Chemistry Chemistry (9th) by Chang 5 21P
Question Details:
Pure nitrogen gas effuses at the rate of 0.311 cm/min while an unknown gas effuses at the rate of 0.133 cm/min under the same conditions. The molecular weight of this gas is
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posted by Sarah21 on 10/24/2008 8:55:46 AM  |  status: Live
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babujoo's comment:
"not correct"
Response Details:
Use Graham's Law of Effusion
 

where:

Rate1 is the rate of effusion of the first gas.
Rate2 is the rate of effusion for the second gas.
M1 is the molar mass of gas 1
M2 is the molar mass of gas 2.
 
Let's say that Nitrogen gas = gas 1  and an unknown gas is gas 2
 
The molar mass of Nitrogen gas (N2)  = 28.01
 
Now we plug in the values into our equation
 
0.311 / 0.133  = √M2  / √28.01
 
√M2  = 12.3756
 
M2  = 1253.155 g/mole
Hope this helps!  Please take the time to rate my answer accordingly.  Thanks! 
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