In many cases corrosion can be effectively controlled by changing or modifying the corrosive environment by: The corrosion nature is reduced by modifying the environment: the removal of harmful constituents in the environment...
Category - Chemistry
The rate and extent of corrosion depends on: Nature of the environment Nature of the metal. S.No Environment based factors Metal based factors 1 Temperature. Position of metal in galvanic series. 2 Humidity. Relative...
There are two types of electrochemical Corrosion: Galvanic corrosion Differential aeration or Concentration cell corrosion Galvanic corrosion When two dissimilar metals are in contact with each other on the presence of aqueous...
Based on the corrosion of metals in the nature of the environment it is classified into two types: Dry or chemical corrosion. Wet or electrochemical corrosion. S.No Dry or chemical corrosion Wet or electrochemical...
Chemistry of Corrosion Most of the metals (except noble metals like gold, platinum etc.) exist in nature as ores (metallic oxide, sulphide, carbonate, silicate etc.). By metallurgical operations, these ores are converted into...
The following are some examples for corrosion that we experience in our day to day life. (i) Rusting of iron : Iron exposed to the environment forms a brown rust film on its surface. (ii) Water stored in aluminium vessel : If...
Here are a few simple electrochemistry solved problems along with their solutions: 1. Calculate the single electrode potential of copper metal immersed in 0.15°MCu2+ solution. E° for copper...
Definition : When elements are arranged in increasing order of their standard reduction electrode potentials, the series so obtained is known as electrochemical (or) electromotive series. or A series in which standard reduction...
Nernst equation can be used to calculate the emf of the cells when the concentration of reactants and products are known. Let us consider a general redox reaction Mn+ + ne– M. For any reversible reaction, the change in...
It is impossible to know the absolute values of the single electrode potential. It is because a single electrode constitutes only a half- cell. A half-cell would not lose or gain electrons by itself. The loss or gain of electrons...
