6. i ii Consider the following half reactions: Write the balanced half-reaction for the oxidation that occurs. Write the balanced half-reaction for the reduction that occurs. iii Write the balanced redox reaction. V Calculate the cell potential. iv Write the potential for each half-reaction next to it (the values are in your text) vi Calculate AG° at 25 °C. vii Is this reaction spontaneous? Why? viii Draw and label the cell for this reaction. Zn²+ + 2e¹- → Zn Fe³+ + 3e¹- → Fe ix Write the line notation for the cell. E° = -0.76 V E = -0.036V DELL

A galvanic (voltaic) cell consists of an electrode composed of nickel in a 1.0 M nickel(II) ion solution and another electrode composed of gold in a 1.0 M gold(III) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Refer to the list of standard reduction potentials. E° V 'cell * TOOLS х10

6. Sketch a voltaic cell for the following overall redox reaction. 3 Cl2(g) + 2 Fe(s) — 6 CІ (аq) + 2 Fe3+(aq) а. Label the anode and cathode b. Indicate the half-reaction occurring at each electrode c. Indicate the species present in each solution.

Consider a voltaic cell that can be described like so. It is set up at standard conditions. A gold electrode is in contact with Au(NO3)3 (aq) and a lead electrode in contact with Pb(NO3)2 (aq) at 25 degrees C. Write true or false next to each of the following statements regarding the voltaic cell. I. Adding H20 to the lead half-cell will increase the measured cell potential. II. A salt-bridge is used to prevent charge buildup in the half-cells. III. This will result in the production of Pb2+ ions.

A galvanic (voltaic) cell consists of an electrode composed of cadmium in a 1.0 M cadmium ion solution and a second electrode composed of lead in a 1.0 M lead(II) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Use this list of standard reduction potentials. E: cell 11 x10 TOOLS V

For a voltaic cell based on the reaction below, what reaction happens at the cathode?Zn(s)+2H+(aq)→Zn2+(aq)+H2(g)   a. Zn(s)→Zn2+(aq)+2e-   b. 2H+(aq)+2e-→H2(g)   c. Zn2+(aq)+2e-→Zn(s)   c. H2(g)→2H+(aq)+2e-

A charger that supplies a current of 120. mA of current is used to recharge a NiCd battery. How much time, in h, does it take to convert 1.55g of Cd(OH)2 back into Cd so the battery can be used again? O4.73 O 1.25 O 2.29 3.94 O0.732