PV = nRT: Understanding Pressure Units in Gas Laws

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SUMMARY

The discussion clarifies that the pressure unit used in the ideal gas law equation PV = nRT depends on the value of the gas constant R. If R is 8.314472 m³·Pa·K⁻¹·mol⁻¹, pressure must be in Pascals (Pa) and volume in cubic meters (m³). Conversely, if R is 0.08205784 L·atm·K⁻¹·mol⁻¹, pressure should be in atmospheres (atm) and volume in liters (L). This distinction is crucial for accurate calculations in gas law applications.

PREREQUISITES
  • Understanding of the ideal gas law (PV = nRT)
  • Familiarity with the gas constant (R) and its different values
  • Knowledge of pressure units: Pascals (Pa) and atmospheres (atm)
  • Basic concepts of volume measurement in cubic meters (m³) and liters (L)
NEXT STEPS
  • Research the implications of using different values of R in gas law calculations
  • Learn about unit conversions between Pascals and atmospheres
  • Explore real-world applications of the ideal gas law in chemistry and physics
  • Investigate the derivation and significance of the ideal gas law
USEFUL FOR

Chemistry students, physics enthusiasts, and professionals in scientific fields who require a solid understanding of gas laws and pressure unit conversions.

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Quick Question...Test at 8 am!

When using PV = nRT does P have to be in atm? Or is it Pa?
 
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BuBbLeS01 said:
When using PV = nRT does P have to be in atm? Or is it Pa?

depends on the R you're using...

if you learned
R = 8.314472 m3·Pa·K-1·mol-1

then you need to use pressure in Pa. and volume needs to be in m^3. which R did you learn?

if you learned
R = 0.08205784 L·atm·K-1·mol-1

then you need to use pressure in atm. and volume needs to be in L.

have a look at the R using different units:

http://en.wikipedia.org/wiki/Ideal_gas_law
 
oh ok thanks
 

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