1. Sketch a construction of a voltaic cell based on the reaction: Cd(s) + Ni ⁺²(aq) => Cd ⁺² (aq) + Ni(s). Label the anode and cathode.Identify the positive and negative electrodes.Indicate the direction of flow of the electrons and ions.

2. Some standard potentials are:

VO₂ ⁺¹ + 2 H ⁺¹ + 1 e ^-1 => VO ⁺² + H₂O E^o = +1.00 v

Fe ⁺³ + 1 e - => Fe ⁺² E^o = +0.77 v

Zn ⁺² +2 e- = Zn E^o = -0.763 v

a) What reagent could you use to reduce Fe ⁺³ ?

b) What is the balanced reaction equation and electrode potential for the Fe ³⁺ reduction reaction?

 3. Refer to a table of potentials and explain the following facts by writing a balance chemical reaction equation and calculating the potential of the reaction:

a) Ag may be recovered from a solution of Ag ⁺¹ ions by using a Cu wire.

b) Cu ⁺² solutions are corrosive to Fe metal devices.

c) Zn covered Fe wire resists corrosion because the oxidation of Zn is favored over Fe.

d) Lead car batteries have Pb anodes and PbO₂ cathodes.

e) Flashlight batteries have Zn anodes and MnO₂ cathodes

f) Electrolysis of a NaCl solution produces three useful products: NaOH, H₂, and Cl₂.

g) Fe ⁺² can catalyze the decomposition of H₂O₂ to O₂ and H₂O because Fe ⁺² can reduce H₂O₂ to H₂O and Fe ⁺³ can oxidize it to O₂.