Calculate the Gibbs free energy change for the following electrochemical reaction at 298 K:Mg(s) + 2H+(aq) → Mg2+(aq) + H2(g)Given:Standard Gibbs free energy change of formation of Mg2+: -466 kJ/molStandard Gibbs free energy change of formation of H+: 0 kJ/molStandard Gibbs free energy change of formation of H2: 0 kJ/molStandard Gibbs free energy change of formation of Mg: 0 kJ/mol

Question

Calculate the Gibbs free energy change for the following electrochemical reaction at 298 K:Mg(s) + 2H+(aq) → Mg2+(aq) + H2(g)Given:Standard Gibbs free energy change of formation of Mg2+: -466 kJ/molStandard Gibbs free energy change of formation of H+: 0 kJ/molStandard Gibbs free energy change of formation of H2: 0 kJ/molStandard Gibbs free energy change of formation o

Answer 1

To calculate the Gibbs free energy change  G  for the reaction, we can use the following equation:G = G products  - G reactants For the reactants, we have Mg s  and 2H+ aq , and for the products, we have Mg2+ aq  and H2 g . Using the given standard Gibbs free energy change of formation values:G reactants  = 0 kJ/mol  Mg  + 2 * 0 kJ/mol  H+  = 0 kJ/molG products  = -466 kJ/mol  Mg2+  + 0 kJ/mol  H2  = -466 kJ/molNow, we can calculate the Gibbs free energy change for the reaction:G = G products  - G reactants  = -466 kJ/mol - 0 kJ/mol = -466 kJ/molSo, the Gibbs free energy change for the given electrochemical reaction at 298 K is -466 kJ/mol.