To calculate the Gibbs free energy change G for the electrochemical reduction of 1 mol of Au3+ to Au, we can use the following equation:G = -nFEwhere:- n is the number of moles of electrons transferred in the redox reaction in this case, 3 moles of electrons, as Au3+ gains 3 electrons to become Au - F is the Faraday constant approximately 96,485 C/mol - E is the cell potential 1.42 V Now, we can plug in the values and calculate G:G = - 3 mol 96,485 C/mol 1.42 V G = -411,293.62 J/molSince the value is negative, the reaction is spontaneous under standard conditions. The Gibbs free energy change for the electrochemical reduction of 1 mol of Au3+ to Au in a standard electrochemical cell with a cell potential of 1.42 V at 298 K is approximately -411,293.62 J/mol.