how many electrons are transfered in one atom of Mn in the reaction?MnO2+4HCl=MnCl2+2H2O+Cl2
To determine how many electrons are transferred in the reaction, we need to examine the oxidation states of manganese (Mn) in both the reactant and product compounds.
In the reactant compound, MnO2, the oxidation state of Mn is +4. (Oxygen has an oxidation state of -2, and since the overall charge of MnO2 is neutral, the oxidation state of Mn must be +4).
In the product compound, MnCl2, the oxidation state of Mn is +2. (Since Cl has an oxidation state of -1 and there are two Cl atoms in MnCl2, the overall charge must be balanced, which makes the oxidation state of Mn +2).
By comparing the oxidation states of Mn in the reactant and product compounds, we can determine the change in oxidation state as the number of electrons transferred.
From +4 to +2, the oxidation state decreases by 2. Each electron carries a charge of -1. Therefore, 2 electrons are transferred during the reaction.
So, in one atom of Mn, 2 electrons are transferred in the given reaction.