Michigan State University

CEM152 - Principles of Chemistry II


deltaGstandcombustion.html

Estimate the standard free energy change for the combustion of methane
CH4(g) + O2(g) -> H2O(g) + CO2(g)
assuming 1 mole of methane consumed. The following thermodynamic data may be useful:

DHof CH4(g) = -74.80 kJ/mol
So CH4(g) = 186.3 J/K-mol
DGof CH4(g) = -50.8 kJ/mol

DHof O2(g) = 0 kJ/mol
So O2(g) = 205.0 J/K-mol
DGof O2(g) = 0 kJ/mol

DHof H2O(g) = -241.8 kJ/mol
So H2O(g) = 188.8 J/K-mol
DGof H2O(g) = -228.6 kJ/mol

DHof CO2(g) = -393.5 kJ/mol
So CO2(g) = 213.6 J/K-mol
DGof CO2(g) = -394.4 kJ/mol


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updated 03mar07 by pfm