MnO4
-
(aq) + 8H+
(aq)+ 5e → Mn2+ (aq)+ 4H2O (l)
explain the process in detail how reaction occur in detail
The given reaction is a redox reaction in which permanganate ion (MnO4-) is reduced to manganese ion (Mn2+), while 8H+ ions are consumed and 5 electrons are gained in the process.
The reaction occurs in an acidic solution, indicated by the presence of the H+ ions. In acidic conditions, the permanganate ion (MnO4-) is able to accept electrons and undergo reduction.
The MnO4- ion gains 5 electrons and is reduced to Mn2+ ion, as shown in the reaction. This reaction is typically carried out in the presence of a reducing agent, such as sulfur dioxide or hydrogen peroxide, which provides the electrons needed for the reduction to occur.
The H+ ions in the solution are consumed in the process, forming water molecules (H2O), as shown in the reaction. The water molecules are produced as a result of the combination of the hydrogen ions with the oxygen atoms from the MnO4- ion.
Overall, the reaction results in the conversion of permanganate ion to manganese ion in the presence of acid and a reducing agent. The reaction involves the transfer of electrons and the formation of water molecules.