Electrochemistry
The study of the production of electricity from energy released during
spontaneous chemical reactions and the use of of electrical energy to
bring about non-spontaneous chemical transformations
spontaneous Non-spontaneous
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Electrochemistry: Principles and Applications, Schemes and Mind Maps of Electrochemistry
A concise introduction to electrochemistry, covering fundamental concepts such as spontaneous and non-spontaneous reactions, electrochemical cells, and standard electrode potentials. It explains the principles behind the conversion of chemical energy to electrical energy and vice versa, using examples like the daniell cell. The document also discusses the activity series and the role of the standard hydrogen electrode as a reference point for measuring electrode potentials. It is a valuable resource for students seeking a basic understanding of electrochemistry.
Typology: Schemes and Mind Maps
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Electrochemistry
The study of the production of electricity from energy released during
spontaneous chemical reactions and the use of of electrical energy to
bring about non-spontaneous chemical transformations
spontaneous Non-spontaneous
Why do we study Electrochemistry?
Production of metals and chemicals by electrochemical methods
Batteries and fuel cells
Transmission of sensory signals through cells to brain
The reactions carried out electrochemically can be energy
efficient and less polluting – ecofriendly technologies
Daniell Cell This cell converts chemical energy liberated during the following redox reaction to electrical energy and has an electrical potential equal to 1.1 V, when the concentration of Zn2+^ and Cu 2+ ions is unity. An oxidation-reduction (redox) reaction is a type of chemical reaction that involves a transfer of electrons between two species.
The two portions of the cell are called Half-cells or Redox Couples
Cell notations It is now accepted convention that while representing the galvanic cell Anode is on the left. Cathode is on the right.
Standard Hydrogen Electrode Standard Hydrogen Electrode is used as a reference electrode when calculating the standard electrode potential of a half cell. The Standard Hydrogen Electrode is often abbreviated to SHE, and its standard electrode potential is declared to be 0 at a temperature of 298K. This is because it acts as a reference for comparison with any other electrode. 2H+^ (aq) + 2e–^ → H 2 (g) Pt(s) ç H 2 (g, 1 bar) ç H+ (aq, 1 M) çç Cu2+ (aq, 1 M)ú Cu is 0.34 V and it is also the value for the standard electrode potential of the half-cell corresponding to the reaction: Cu2+ (aq, 1M) + 2 e– ® Cu(s) Pt(s) ç H 2 (g, 1 bar) ç H+ (aq, 1 M) çç Zn2+ (aq, 1M) ç Zn is -0.76 V corresponding to the standard electrode potential of the half-cell reaction: Zn2+ (aq, 1 M) + 2e– ® Zn(s)
Activity Series
Reducing Agent
Cell Potential
Construct A Galvanic Cell
0.77 V
-0.76 V
Cell Reaction Cell Potential
Spontaneity and Redox reaction
Voltage as an Intensive Property