A)Describe the difference between galvanic and electrolytic cells B)Explain why

Question

A)Describe the difference between galvanic and electrolytic cells

B)Explain why it is generally more preferred to use a three electrode system (composed of working, counter, and reference electrodes) than a two electrode system in electrochemical analysis. Also explain the role of working, counter, and reference electrodes, respectively, in a three electrode system.

C) Polarography is a subclass of voltammetry where the working electrode is a dropping mercury (Hg) electrode (DME). Despite the toxicity of Hg, polarography is getting more widely used due to its unique advantages. List and explain the two major advantages of DME in electroanalytical techniques.

D) The glass electrode used to accurately measure pH is the most common ion-selective electrode. At extreme pH conditions (i.e., strongly acidic and basic conditions), however, they exhibit a significant error in the pH measurement. Explain the origin of this error (5 pt).

Please write in detail and accurately.

Explanation / Answer

Galvanic cell or Electrochemical cell

A galvanic cell is also called an electrochemical cell which converts chemical energy to electrical energy. i.e as a result of chemical reaction, electricity generates.

Example: electrical battery

An electrolytic cell converts electrical energy to chemical energy, i.e on supply of electric current, chemical reaction occurs.

Example: Decomposition of water in to H2 and O2

Electroplating of Cu, Ag etc.

Galvanic cell or Electrochemical cell

Electrolytic cell

A galvanic cell is also called an electrochemical cell which converts chemical energy to electrical energy. i.e as a result of chemical reaction, electricity generates.

Example: electrical battery

An electrolytic cell converts electrical energy to chemical energy, i.e on supply of electric current, chemical reaction occurs.

Example: Decomposition of water in to H2 and O2

Electroplating of Cu, Ag etc.

A spontanious redox reaction occurs in this cell, resulting current production. Here, the redox reaction is not spontanious, hence electricity is supplied to start a chemical reaction. The two half cells are kept in separate coniainer connected by salt bridge or porous partition. Both the halfcells are kept in one container containing solution of molten electrolyte . Here the positvly charged electrode is cathode where reduction occurs, and the negativly charged electrode is anode where oxidation occurs. In this system, the positivly charged electrode is considered to be anode, where oxidation occurs, and the negativly charged electrode is considered to be cathode where reduction occours. In this cell, the species which gets oxidized supplied electrons, which moves from anode to cathode through external circuit. In this cell, the elctron is supplied by the external power supply device (battetry), which enters through cathode and come out through anode.

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