Question

Calculate the Gibbs free energy change (ΔG) for the reaction below at 298 K given the following standard Gibbs free energy of formation data: 2H2(g) + O2(g) → 2H2O(l) ΔG°f (kJ/mol): H2(g) = 0 O2(g) = 0 H2O(l) = -237.14

Answer 1

To calculate the Gibbs free energy change  G  for the reaction, we can use the following equation:G =  Gf_products  -  Gf_reactants For the given reaction:2H2 g  + O2 g   2H2O l The products are 2 moles of H2O l , and the reactants are 2 moles of H2 g  and 1 mole of O2 g .Using the given standard Gibbs free energy of formation data:Gf  kJ/mol :H2 g  = 0O2 g  = 0H2O l  = -237.14We can now plug these values into the equation:G = [2   -237.14 ] - [ 2  0  +  1  0 ]G =  -474.28  - 0G = -474.28 kJ/molThe Gibbs free energy change  G  for the reaction is -474.28 kJ/mol.