Constant Volume Gas thermometer

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SUMMARY

The discussion centers on the use of different gases—nitrogen, oxygen, and hydrogen—in a constant volume gas thermometer. It concludes that while the pressure ratio (P1/P2) at two fixed temperatures (melting ice and boiling water) varies slightly with the type of gas, reducing the gas density leads to a convergence of the pressure ratio towards a uniform value. This behavior aligns with the principles of ideal gas laws, where molecular interactions and volume occupancy become negligible.

PREREQUISITES
  • Understanding of gas laws, specifically the ideal gas law.
  • Knowledge of thermodynamic principles, particularly temperature and pressure relationships.
  • Familiarity with the concept of density and its effects on gas behavior.
  • Basic comprehension of experimental setups for measuring gas properties.
NEXT STEPS
  • Research the ideal gas law and its applications in thermometry.
  • Explore the effects of gas density on pressure measurements in thermodynamic systems.
  • Investigate the properties of different gases and their behavior under varying conditions.
  • Learn about the calibration methods for constant volume gas thermometers.
USEFUL FOR

Students and professionals in physics, engineering, and thermodynamics, particularly those interested in temperature measurement and gas behavior in scientific experiments.

LukeeVassallo
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Hi,

Does it make a difference if you use nitrogen gas or oxygen gas or hydrogen gas in the bulb ? Or they all give the same readings given that an arbitrarily chosen constant if found for each ?

Many Thanks! :)
 
Science news on Phys.org
is found for each* - sry my bad
 
Suppose that P1 and P2 are the pressures of the gas in the bulb at two fixed point temperatures (e.g.pure melting ice and steam above water boiling at standard pressure. We find that the ratio P1/P2 does depend slightly on the gas in the bulb, but if we reduce the density of the gases, the ratio converges towards the same value whatever gas we use. We are approaching an 'ideal' gas (because the attractive forces between molecules, and the fraction of container space taken up by the molecules themselves are becoming negligible).
 

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