Calculating Mass of Helium Gas at STP

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SUMMARY

The calculation of the mass of helium gas (He) occupying 8.5 liters at standard temperature and pressure (STP) was discussed, utilizing the ideal gas law equation PV = nRT. The correct calculation yields 10.6 grams of helium, derived from the formula n = PV/RT, where pressure (P) is 101 kPa, volume (V) is 8.5 L, the ideal gas constant (R) is 8.3145, and temperature (T) is 273 K. The confusion arose from a comparison with the solutions manual, which incorrectly stated the mass as 1.52 grams.

PREREQUISITES
  • Understanding of the Ideal Gas Law (PV = nRT)
  • Knowledge of standard temperature and pressure (STP) conditions
  • Familiarity with unit conversions (liters to moles)
  • Basic principles of gas behavior and molar mass calculations
NEXT STEPS
  • Review the Ideal Gas Law applications in various scenarios
  • Learn about molar mass calculations for different gases
  • Explore the significance of STP in gas calculations
  • Investigate common errors in gas law calculations and how to avoid them
USEFUL FOR

Students in chemistry, educators teaching gas laws, and anyone involved in scientific calculations related to gases will benefit from this discussion.

kasse
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[SOLVED] Mass of gas

Homework Statement



What mass of He gas occupies 8.5 L at 273 K and 1 atm?

Homework Equations



PV = nRT

The Attempt at a Solution



n = PV/RT = (101 kPa * 8.5 L)/(8.3145 * 273 K) = 2.64E-3 mol --> 10.6 g

My solutions manual says 1.52 g. Am I right or wrong?
 
Physics news on Phys.org
2.64E-3 mole? Really? I seem to remember a mole of gas at STP is 22.4 liters. What does a mole of helium mass? The book is right.
 

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