Advanced Electrochemistry Tutorial 2

1) A constant current of 0.800 A was used to deposit copper at the cathode and oxygen at the anode of an electrolytic cell. Calculate the mass of each product that was formed in 15.2 min, assuming that no other redox reactions occur. (0.24 g of Cu and 0.0605 g of O2)

2) Briefly explain how potentiometric method can be used to quantify concentration of Mn+ ions.

3) Why is not advisable to use two electrodes system when perform voltammetric experiment

4) In a cyclic voltammetry experiment, what is meant by “diffusion control measurement

5) What kinds of chemical information can be obtained from a cyclic voltammogram.

6) Briefly explain why is the electrochemical ‘efficiency’ lower than the 100% theoretical maximum

7) Charge is forced through a cell to perform the electrode reaction,Zn2+ + 2e- → Zn. Previous experiments revealed the reaction has a faradaic efficiency of 77.1 %. Given this efficiency, calculate the overall charge passed, by considering that 10-4 mole of zinc metal forms.

8) Explain very briefly the Nernst Layer (Depletion Layer)9) Given below is a cyclic votamograme obtained for reaction

O + ne → R

Briefly describe the important features of the following cyclic voltammogram of the above reaction.

10) Why stripping methods in electroanalytical chemistry is important when analying trace amount of analyte.