Statistical Thermodynamics and Rate Theories/Data

Molecule (K) (K) H2http://webbook.nist.gov/cgi/cbook.cgi?ID=1333-74-0 87.547 6332.52 N2http://webbook.nist.gov/cgi/cbook.cgi?ID=C7727379&Mask=1000#ref-1 2.0518 3393.54 O2http://webbook.nist.gov/cgi/cbook.cgi?ID=C7782447&Mask=1000#Diatomic 2.0793 2273.60 F2http://webbook.nist.gov/cgi/cbook.cgi?Name=fluorine&Units=SI&cDI=on#Diatomic 1.2808 1318.87 HFhttp://webbook.nist.gov/cgi/cbook.cgi?ID=C7664393&Mask=1000#Diatomic 41.345 5954.27 HClhttp://webbook.nist.gov/cgi/cbook.cgi?ID=C7647010&Mask=1000#Diatomic 15.240 4303.41 NOhttp://webbook.nist.gov/cgi/inchi?ID=C10102439&Mask=1000#Diatomic 2.4524 2739.79 C2H2E. Plyler, E. Tidwell, and T. Wiggins, (1963). Rotation-Vibration Constants of Acetylene. Journal of Optical Society America. Table 4, Data section in appendix 1.7012 Example Calculate the ground state characteristic rotational () and characteristic vibrational () temperatures for molecular hydrogen, H2. Where is the reduced Planck constant, is the internuclear distance for ground state hydrogen, is the Boltzmann constant, and is the reduced mass. The characteristic vibrational temperature () is calculated using the following equation Where is Planck's constant, is the Boltzmann constant, and is the vibrational frequency of the molecule. To retain units of K the vibrational frequency must be changed to units of s-1. References