Question

Calculate the standard Gibbs free energy change (ΔG°) for the reaction below at 298 K:2NO(g) + O2(g) → 2NO2(g)Given:ΔG°f(NO2(g)) = -51.29 kJ/molΔG°f(NO(g)) = 86.67 kJ/molΔG°f(O2(g)) = 0 kJ/mol

Answer 1

To calculate the standard Gibbs free energy change  G  for the reaction, we can use the following equation:G =  Gf products  -  Gf reactants For the given reaction:2NO g  + O2 g   2NO2 g G = [2  Gf NO2 g  ] - [2  Gf NO g   + Gf O2 g  ]Now, we can plug in the given values:G = [2   -51.29 kJ/mol ] - [2   86.67 kJ/mol  + 0 kJ/mol]G =  -102.58 kJ/mol  -  173.34 kJ/mol G = -275.92 kJ/molThe standard Gibbs free energy change  G  for the reaction is -275.92 kJ/mol.