In the balanced acidic-medium reaction MnO 4 − + Fe 2+ + H + → Mn 2+ + Fe 3+ + H 2 O, the mole ratio of MnO 4 − to Fe 2+ is:

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In the balanced acidic-medium reaction MnO4− + Fe2+ + H+ → Mn2+ + Fe3+ + H2O, the mole ratio of MnO4− to Fe2+ is:

Answer: 1 : 5.

A 1 : 5
B 1 : 3
C 1 : 6
D 1 : 2

Correct answer: A. 1 : 5

Explanation: MnO4− gains 5 electrons while each Fe2+ loses 1; balancing electrons needs 5 Fe2+ per MnO4−.

Electron transfer in a redox reaction: zinc loses electrons (oxidised, acts as reducing agent) and copper(II) ions gain those same electrons (reduced, acts as oxidising agent).

Concept context

Master electron transfer in chemistry: assign oxidation states, balance half-reactions, identify oxidising and reducing agents, and connect redox to everyday reactions.

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In the balanced acidic-medium reaction MnO<sub>4</sub><sup>−</sup> + Fe<sup>2+</sup> + H<sup>+</sup> → Mn<sup>2+</sup> + Fe<sup>3+</sup> + H<sub>2</sub>O, the mole ratio of MnO<sub>4</sub><sup>−</sup> to Fe<sup>2+</sup> is:

Concept context

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