Question

Calculate the Gibbs free energy change for the combustion of methane gas to produce carbon dioxide and water vapor at a temperature of 298K and a pressure of 1 atm, given the equation:CH4(g) + 2O2(g) -> CO2(g) + 2H2O(g)    ΔG°f = -394.36 kJ/mol (CO2);  ΔG°f = -237.13 kJ/mol (H2O); ΔG°f = -50.8 kJ/mol (CH4);   ΔG°f = 0 kJ/mol (O2)

Answer 1

To calculate the Gibbs free energy change  G  for the combustion of methane, we can use the following equation:G =  Gf products  -  Gf reactants where Gf represents the standard Gibbs free energy of formation for each species involved in the reaction.For the given reaction, we have:G = [1   -394.36 kJ/mol  + 2   -237.13 kJ/mol ] - [1   -50.8 kJ/mol  + 2  0 kJ/mol]G =  -394.36 - 474.26 + 50.8  kJ/molG = -817.82 kJ/molSo, the Gibbs free energy change for the combustion of methane gas to produce carbon dioxide and water vapor at a temperature of 298K and a pressure of 1 atm is -817.82 kJ/mol.