Vol-4 Issue-4 2018 IJARIIE-ISSN(O)-2395-4396 8984 www.ijariie.com 1092 Studies on Redox Equilibrium and Electrode Potentials Bapy Guh 1 , Fakhrul Islam 2 and K. A. Khan 3 1 Department of Physics, Jahangirnagar University,Savar,Dhaka,Bangladesh 2 Department of Physics, Jahangirnagar University,Savar,Dhaka,Bangladesh. 3* Department of Physics, Jagannath University, Dhaka-1100, Bangladesh ( 3* - Corresponding Author) Abstract Metal corrosion is very important factor for redox reaction during cell reactions. So that it has been studied in this research work. When metals react, they give away electrons and form positive ions. This particular topic describes how a metal form hydrated ions in solution. It can be considered the case of Magnesium and Copper in water. It can be compared the following two reactions how these two changes take place: Mg (S) Mg 2+ (aq) + 2e - Cu (S) Cu 2+ (aq) + 2e - It is known that magnesium is more reactive than copper. The first reaction happens much more readily than the second one. Now it will be tried to express this with some numbers. Keywords: Battery, Cell , Electrode, Magnesium Electrode, Copper Electrode, EMF I.Introduction Let us consider a bar of magnesium in a beaker of water. There will be some tendency for the magnesium atoms to oxidized and leave electrons and go into solution as magnesium ions. The electrons will be left behind on the magnesium bar[1-24]. Fig.1: Magnesium in a beaker of water (a). In a very short time, electrons will be a build-up on the magnesium bar and it will be surrounded in the solution by a layer of positive ions[25-45]. These will tend to stay close because they are attracted to the negative charge of electrons on the piece of metal. Some of them will be attracted enough that they will reclaim their electrons and stick back on to the piece of metal.