Question

Calculate the standard free energy change (ΔG°) for the following redox reaction: Zn (s) + 2H+ (aq) → Zn2+ (aq) + H2 (g)Given: ΔG°f (Zn2+) = -153.9 kJ/mol ΔG°f (H+) = 0 kJ/mol ΔG°f (H2) = 0 kJ/mol ΔG°f (Zn) = 0 kJ/mol

Answer 1

To calculate the standard free energy change  G  for the redox reaction, we can use the following equation:G =  Gf products  -  Gf reactants For the given reaction:Zn  s  + 2H+  aq   Zn2+  aq  + H2  g The products are Zn2+  aq  and H2  g , and the reactants are Zn  s  and 2H+  aq .Now, we can plug in the given values for the standard free energy of formation  Gf  for each species:G = [ 1  Gf  Zn2+   +  1  Gf  H2  ] - [ 1  Gf  Zn   +  2  Gf  H+  ]G = [ 1  -153.9 kJ/mol  +  1  0 kJ/mol ] - [ 1  0 kJ/mol  +  2  0 kJ/mol ]G =  -153.9 kJ/mol  -  0 kJ/mol G = -153.9 kJ/molSo, the standard free energy change  G  for the given redox reaction is -153.9 kJ/mol.