2MnO4 + H + 5HSO3 = 2Mn + 5HSO4 + 3H2O
Which is being oxidized and which is being reduced?
hopefully Writeteacher actually says the answer smh
I hope so. I need this question answered for my homework that is due tonight.
To determine which species is being oxidized and which species is being reduced in a chemical reaction, you can follow these steps:
1. Assign oxidation numbers to each atom in the reactants and products.
Oxidation number is a number assigned to each atom in a molecule or ion to indicate its degree of oxidation or reduction in a chemical compound.
2Mn7+ O4- + H+ + 5H+ S+5 O3- = 2Mn2+ + 5H+ S+6 O4- + 3H2O
In the given reaction, we can see the changes in the oxidation numbers for each element:
2Mn: goes from +7 to +2, a decrease in oxidation number (reduction)
O in MnO4: remains at -2, no change
H: goes from +1 to +1, no change
H in HSO3: goes from +1 to +1, no change
S in HSO3: goes from +4 to +6, an increase in oxidation number (oxidation)
O in HSO3: goes from -2 to -2, no change
2. Identify the species whose oxidation number decreases; this is the substance being reduced. In this case, Manganese (Mn) is being reduced from +7 to +2, which means it is gaining electrons and being reduced.
3. Identify the species whose oxidation number increases; this is the substance being oxidized. In this case, Sulfur (S) is being oxidized from +4 to +6, which means it is losing electrons and being oxidized.
Therefore, in the reaction:
Manganese (Mn) is being reduced, and Sulfur (S) is being oxidized.