Related Experiment Video
Updated: Jan 2, 2026

A Simple, Low-cost, and Robust System to Measure the Volume of Hydrogen Evolved by Chemical Reactions with Aqueous Solutions
Published on: August 17, 2016
Second and Third Virial Coefficients for Hydrogen
R D Goodwin1, D E Diller1, H M Roder1
1Cryogenic Engineering Laboratory, National Bureau of Standards, Boulder, Colo.
Second and third virial coefficients for parahydrogen were calculated using precise PVT data. These results align with existing data and provide analytical formulas for thermodynamic calculations.
Area of Science:
- Thermodynamics
- Physical Chemistry
- Statistical Mechanics
Background:
- Accurate thermodynamic data is crucial for understanding gas behavior.
- Virial coefficients describe deviations from ideal gas laws.
Purpose of the Study:
- To derive second and third virial coefficients for parahydrogen.
- To develop analytical representations for thermodynamic calculations.
Main Methods:
- Utilized closely spaced Pressure-Volume-Temperature (PVT) data.
- Analyzed data from 24 to 100 K for virial coefficient derivation.
- Developed analytical formulas for combined data (20-423 K).
Main Results:
- Successfully derived second and third virial coefficients for parahydrogen.
- Demonstrated good agreement with published data for normal hydrogen at 100 K.
- Presented analytical representations of the virial coefficients.
Conclusions:
- The derived virial coefficients are reliable for parahydrogen.
- The analytical formulas can aid in computing thermodynamic functions.
- The findings relate to theoretical models like the Lennard-Jones potential.
More Related Videos
14:11Quantification of Hydrogen Concentrations in Surface and Interface Layers and Bulk Materials through Depth Profiling with Nuclear Reaction Analysis
Published on: March 29, 2016
12:11Computation of Atmospheric Concentrations of Molecular Clusters from ab initio Thermochemistry
Published on: April 8, 2020
Related Concept Videos
Real Gases: Effects of Intermolecular Forces and Molecular Volume Deriving Van der Waals Equation
Heat Capacities of an Ideal Gas III
Van der Waals Equation
First, the attractive forces between molecules, which are stronger at higher densities and reduce the pressure, are considered by adding to the pressure a term equal to the square of the molar density multiplied by a positive coefficient a. Second, the volume...
Heat Capacities of an Ideal Gas II
Spin–Spin Coupling: Three-Bond Coupling (Vicinal Coupling)
The extent of coupling depends on the C‑C bond length, the two H‑C‑C angles, any electron-withdrawing substituents, and the dihedral angle between the involved orbitals. The...
Hydrogen Bonds
Hydrogen Bonds Control the World!
Because hydrogen has very weak electronegativity when it binds with a strongly electronegative atom, such as oxygen or nitrogen, electrons in the bond are unequally shared....