Final answer:
In the redox reaction, 10 moles of electrons are transferred as each Mn atom in MnO4- gains 5 electrons to form Mn2+ and there are 2 moles of MnO4-.
Step-by-step explanation:
The question asks how many moles of electrons are transferred in the reduction-oxidation reaction provided. In the given reaction, MnO4- is reduced to Mn2+. The oxidation state of Mn in MnO4- is +7, and it changes to +2 in Mn2+. Therefore, each Mn atom gains 5 electrons during the reduction process. Since there are 2 moles of MnO4- each gaining 5 electrons, the total number of moles of electrons transferred is 2 moles of MnO4- × 5 electrons/Mn = 10 moles of electrons.
The balanced redox reaction given is:
2 MnO₄⁻(aq) + 10 Br⁻(aq) + 16 H⁺(aq) → 2 Mn²⁺ (aq) + 5 Br₂ (aq) + 8 H₂O(l)
In this reaction, MnO₄⁻ is reduced to Mn²⁺.
For each MnO₄⁻ ion, 5 moles of electrons are transferred.
Therefore, for 2 MnO₄⁻ ions, the total moles of electrons transferred (n) is 2 x 5 = 10 moles of electrons.