Calculate the standard cell potential and the standard free-energy change (in kilojoules) for the reaction below. (See Appendix D for standard reduction potentials.) <QUESTION REFERENCES APPENDIX D>

The standard cell potential (E°) is the measure of the voltage produced by an electrochemical cell under standard conditions (1 M concentration, 1 atm pressure, and 25°C). It is calculated using the standard reduction potentials of the half-reactions involved in the cell. A positive E° indicates a spontaneous reaction, while a negative E° suggests non-spontaneity.

The standard free energy change (ΔG°) quantifies the spontaneity of a reaction at standard conditions. It is related to the standard cell potential by the equation ΔG° = -nFE°, where n is the number of moles of electrons transferred and F is Faraday's constant (approximately 96485 C/mol). A negative ΔG° indicates that the reaction is spontaneous.

Half-reactions represent the oxidation or reduction processes occurring in an electrochemical cell. Each half-reaction has an associated standard reduction potential, which indicates the tendency of a species to gain electrons. By combining the half-reactions and their potentials, one can determine the overall cell potential and the direction of electron flow in the cell.