MnO4(aq) + 8H + (aq) + 5Fe2+ → Mn2+(aq) + 4H2O(I). The oxidation number of manganese in the above reaction changed from?
Answer Details
In the given chemical reaction, MnO4- ion is reduced to Mn2+ ion, indicating a decrease in the oxidation number of manganese. To determine the change in oxidation number, we need to know the oxidation state of manganese in the reactant and product side. In MnO4-, oxygen has an oxidation state of -2, so the oxidation state of Mn can be calculated as follows: (+4) + 4(-2) = -8 x + (-8) = -1 (the net charge of MnO4-) Solving for x, the oxidation state of Mn in MnO4- is +7. On the product side, there are two H2O molecules, so the oxidation state of Mn can be calculated as follows: x + 4(+2) + 2(-2) = 0 (the net charge of Mn2+) Solving for x, the oxidation state of Mn in Mn2+ is +2. Therefore, the oxidation state of Mn changes from +7 to +2 in the given reaction, which means that the correct answer is "+7 to +2".