Calculate and write the quotient (4 – i)/(3 + 2i) in the a + bi form.

The Gibbs free energy change for a reaction can be calculated using the formula: ?G = -nFE where n is the number of moles of electrons transferred in the reaction, F is Faraday's constant (96,485 C/mol), and E is the cell potential. In this case, the balanced equation shows that 3 moles of electrons are transferred, so n = 3. Using the given cell potentials, we can calculate the standard cell potential: E°cell = E°reduction (cathode) - E°oxidation (anode) E°cell = 0.80 V - (-1.66 V) E°cell = 2.46 V Now, we can calculate the standard Gibbs free energy change using the formula: ?G° = -nFE°cell ?G° = -(3 mol)(96,485 C/mol)(2.46 V) ?G° = -7.17 x 10^5 J/mol Converting this to kilojoules per mole gives: ?G° = -717 kJ/mol Therefore, the standard Gibbs free energy change (?G°) for the reaction is -717 kJ/mol. This negative value indicates that the reaction is spontaneous (exothermic) under standard conditions.