What is the mass of a gas sample at STP?

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SUMMARY

The mass of a gas sample at Standard Temperature and Pressure (STP) can be calculated using the ideal gas law. At STP, one mole of an ideal gas occupies 22.4 liters. Therefore, a gas sample occupying 44.8 liters corresponds to 2 moles. Given that the atomic mass of helium (He) is 4 grams per mole, the mass of the gas sample is 8 grams, not 4 grams as initially assumed.

PREREQUISITES
  • Understanding of the ideal gas law
  • Knowledge of molar volume at STP (22.4 L)
  • Familiarity with Avogadro's number (6.02 x 1023)
  • Basic concepts of atomic mass and molar mass
NEXT STEPS
  • Study the ideal gas law and its applications
  • Learn how to calculate moles from volume at STP
  • Explore the concept of molar mass and its significance
  • Investigate real gas behavior compared to ideal gas assumptions
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Students in chemistry, educators teaching gas laws, and anyone interested in understanding the properties of gases at STP.

Dx
Hi!

A simple He occupies 44.8L at STP. what is the mass of the sample?

my answer was 4g since the atomic mass is 4u but I am wrong. someone/anyone enlighten me towards the right path so I may be one again.
Thanks!
Dx :wink:
 
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44.8 L at STP is how many moles?
 
Originally posted by Bystander
44.8 L at STP is how many moles?

I donno? the question doesn't say. nor can i find out how to compute that since i don't have the mass.
 
Somewhere in the text or lectures for your course, it has been stated, " One mole of an ideal gas occupies 22.4 L at STP." If it ain't been said outright to you previously, it has now. One mole also contains Avogadro's number of molecules, 6.02x10E23. This should have you in business on this and your other posted question. If not, holler.
 

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