Question

Calculate the standard free energy change for the following redox reaction:2HgO(s) → 2Hg(l) + O2(g)Given: ΔG°f (HgO) = -90.83 kJ/molΔG°f (Hg) = 0 kJ/mol ΔG°f (O2) = 0 kJ/mol.

Answer 1

To calculate the standard free energy change  G  for the given redox reaction, we can use the following equation:G =  Gf products  -  Gf reactants For the products:2 moles of Hg l  have a Gf of 0 kJ/mol, so the total Gf for Hg l  is 2 * 0 = 0 kJ.1 mole of O2 g  has a Gf of 0 kJ/mol.For the reactants:2 moles of HgO s  have a Gf of -90.83 kJ/mol, so the total Gf for HgO s  is 2 * -90.83 = -181.66 kJ.Now, we can plug these values into the equation:G =  0 + 0  -  -181.66  = 181.66 kJSo, the standard free energy change for the given redox reaction is 181.66 kJ.