After balancing the following reaction under acidic conditions , how many electrons are transferred?
Mn²⁺ (aq) + BiO₃^{1 -} (aq) →Bi³⁺ (aq) + MnO₄^{1 -} (aq) [Acidic conditions]

Question

After balancing the following reaction under acidic conditions , how many electrons are transferred? Mn²⁺ (aq) + BiO₃^{1 -} (aq)→Bi³⁺ (aq) + MnO₄^{1 -} (aq) [Acidic conditions]

Quizplus · Accepted Answer

In the given reaction, Mn goes from a +2 oxidation state in Mn2+ to a +4 oxidation state in MnO2, losing 2 electrons in the process. Bi goes from a +3 oxidation state in BiO+ to a +5 oxidation state in Bi3+, losing 2 electrons. The sulfur atoms in the reactants and products do not change their oxidation states; thus, they do not contribute to the electron transfer in this reaction. Therefore, the total number of electrons transferred in the reaction is 2 (from Mn) + 2 (from Bi) = 4. However, without the specific details of the oxidation states of each element in the given compounds due to the formatting (^2,, etc.), a precise calculation cannot be made based on the provided information. The correct calculation involves identifying the changes in oxidation states of all elements involved and summing the total electrons transferred. Given the error in interpreting the specific details due to formatting, the correct answer based on standard redox reaction analysis principles cannot be accurately determined without the correct interpretation of the chemical species involved.

After Balancing the Following Reaction Under Acidic Conditions , How