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Form 4 Chemistry lessons on electrochemistry
Components of the Hydrogen half – cell
(7m 32s)
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1.
Meaning of electrochemistry and electrochemical reactions
2.
An experiment to determine displacement reactions among metals
3.
Comparison between the Strength of reducing and oxidizing agents
4.
Meaning, importance and examples of oxidation numbers
5.
Rules in assigning oxidation numbers with examples
6.
An experiment to demostrate Redox reactions involving Halide ions and halogens
7.
Order of oxidizing power for halogens.
8.
Examples of redox reactions
9.
Reaction of heated Iron with dry chlorine
10.
How reaction between Bromine and Iron (II) ions takes place
11.
How Oxidation by potassium Manganate (VII) (KMnO4) take place
12.
Action of potassium dichromate (VI) on iron (II) ions (#Fe^(2+)#):
13.
Action of acidified potassium permanganate on hydrogen Peroxide.
14.
Oxidation of iron (II) salts by #H_2O_2# and terms used for describing oxidation
15.
Electrochemical cell:The tendency of metals to form ions
16.
Experiment to measure the relative tendency of metals to ionize and the roles of salt bridge in an electrochemical cell
17.
Cell diagram for a voltaic cell;rules or conventions for cell representation
18.
Positive and negative E values of an electrochemical cell with examples
19.
Meaning of The standard electrode potential (#Etheta# ) and its importance
20.
The standard Hydrogen Electrode
21.
Components of the Hydrogen half – cell
22.
Negative and positive electrode potentials
23.
Examples of Standard electrode potentials reduction potentials
24.
Uses of standard electrode potential
25.
How to calculate the electrode potential value for REDOX reaction with examples
26.
Voltaic cells:Types of electrochemical cells
27.
Primary cells or dry cells structure, chemical reaction and functions of the various of its components.
28.
Meaning of secondary cells and the chemical reactions that take place
29.
Meaning, structure and chemical reactions of fuel cells
30.
Meaning and terminologies used in electrolysis
31.
Preferential discharge of ions during electrolysis
32.
How electrolysis of dilute sulphuric (VI) acid (#H_2SO_4#) occurs
33.
How electrolysis of dilute sodium chloride occurs
34.
How electrolysis of brine or concentrate sodium chloride takes place
35.
How Electrolysis of Copper (II) Sulphate solution takes place
36.
Factors affecting electrolysis and electrolytic products.
37.
Applications of electrolysis
38.
Manufacture of sodium hydroxide, chlorine and hydrogen;Advantages of mercury cathode cell and disadvantages of mercury cathode cell
39.
Uses of sodium hydroxide, chlorine, and hydrogen
40.
Quantitative aspects of electrolysis
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