Stable Bonds at Room Temperature

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SUMMARY

The discussion focuses on calculating the temperature at which the average kinetic energy of helium atoms equals the bond energy of the van der Waals bond in He2, specifically 7.9 x 10-4 eV. The calculation involves converting the bond energy to joules and using the equation (3/2)kbT, where kb represents Boltzmann's constant. The value of kb is determined to be 2.829 x 10-25 J. The main challenge highlighted is the need to derive the temperature from the given energy value.

PREREQUISITES
  • Understanding of ideal gas laws and kinetic theory
  • Knowledge of Boltzmann's constant (kb) and its significance
  • Ability to convert energy units from eV to joules
  • Familiarity with basic thermodynamic equations
NEXT STEPS
  • Research the properties of van der Waals forces in noble gases
  • Learn about the implications of kinetic energy in gas behavior
  • Explore the calculation of temperature from energy in thermodynamics
  • Study the applications of Boltzmann's constant in statistical mechanics
USEFUL FOR

This discussion is beneficial for physics students, researchers in thermodynamics, and anyone interested in the molecular behavior of gases at varying temperatures.

PeachBanana
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Homework Statement


We know that the average kinetic energy of an ideal gas atom or molecule at Kelvin temperature T is (3/2)kbT. For what temperature T_He does the average kinetic energy of an ideal gas atom or molecule equal the bond energy of the van der Waals bond in He_2 7.9*10^-4 ev?

Homework Equations



(3/2) kb * T


The Attempt at a Solution



7.9*10^-4 ev * 1.602*10^-19 J = 1.265*10^-22 J

(3/2) * kb * 298 K = 1.265*10^-22 J

kb = 2.829*10^-25 J

The answer asks for a temperature and I have an energy. I was really unsure about this one.
 
Physics news on Phys.org
Hello. kb stands for "Boltzmann's constant" and has a value that you can find in your text. Looks like you assumed room temperature, but the temperature is what you want to determine.
 

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