Gibbs Free Energy of Atomic Hydrogen Ionization

[ientist]

Homework Statement

Despite extensive searches of the web and my old honors freshman chem text, I have yet to find a kj /mol value for either the standard Gibbs' Free Energy (Delta-G-naught (298° K)) or standard ENTROPY (Delta-S-naught) for the ionization of gaseous ATOMIC Hydrogen (or for the reverse process; gaseous atomic Hydrogen formation from free protons and electrons)

Thanks in Advance

Homework Equations

The Attempt at a Solution

I can readily find reference to the 1312 kj/mol Ionization "Energy" (ENTHALPY (Delta-H-naught)) but I need the Gibbs free energy for comparisons, or at least the standard entropy change from which I can calculate Delta-G-naught

 

[mark726]

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Hello, thank you for reaching out. The standard Gibbs free energy and standard entropy values for the ionization of gaseous atomic hydrogen can be found in various sources. The standard Gibbs free energy for this process is -1312 kJ/mol, which is the same value as the ionization energy you have mentioned. The standard entropy value for this process is 130.68 J/molK. These values can be found in standard thermodynamic tables or in online databases such as NIST Chemistry WebBook. I hope this helps with your calculations.