Multiple Choice
What is the oxidation number of each underlined element?
a) P4 b) BO33– c) AsO42– d) HSO4–
20. Electrochemistry
Standard Reduction Potentials
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Determine the total number of electrons transferred in the following balanced reaction.
4 MnO4– (aq) + 12 H3O+ (aq) → 4 Mn2+ (aq) + 5 O2 (g) + 18 H2O (g)
A
4
B
6
C
12
D
16
E
20
Verified step by step guidance1
Identify the oxidation states of manganese in the reactants and products. In MnO4−, manganese is in the +7 oxidation state, and in Mn2+, it is in the +2 oxidation state.
Calculate the change in oxidation state for manganese. The change is from +7 to +2, which means each manganese atom gains 5 electrons.
Determine the number of MnO4− ions involved in the reaction. The balanced equation shows 4 MnO4− ions.
Multiply the number of electrons gained per manganese atom by the number of MnO4− ions. This is 5 electrons per manganese atom times 4 MnO4− ions.
Sum the total number of electrons transferred. The total number of electrons transferred is the product from the previous step.
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