Question detail
Balance the following redox equation: MnO₄⁻ + Fe²⁺ → Mn²⁺ + Fe³⁺. What are the oxidation states of manganese and iron in the reactants and products?
Try the question, check the answer, then read the explanation to understand the curriculum point.
At a glance
Question
Type
exam_style
Style
Topic
Oxidation, reduction and redox equations
Question
Balance the following redox equation: MnO₄⁻ + Fe²⁺ → Mn²⁺ + Fe³⁺. What are the oxidation states of manganese and iron in the reactants and products?
Answer
MnO₄⁻ + 5Fe²⁺ → Mn²⁺ + 5Fe³⁺; Oxidation state of Mn changes from +7 to +2, and Fe changes from +2 to +3.
Explanation
This answer is strong as it provides a balanced equation and correctly identifies the oxidation states of manganese and iron before and after the reaction. The question assesses the ability to balance redox equations and understand oxidation state changes.
Common mistake
Balancing Redox Equations Mistake
Students often forget to balance both the number of atoms and the charges in redox equations, leading to incorrect final equations.
To balance a redox equation, first separate the oxidation and reduction half-equations. Ensure that both the number of atoms and the total charge are equal on both sides. For example, in the half-equation for the reduction of MnO4- to Mn2+, balance the manganese and oxygen atoms, then balance the charges by adding electrons. This ensures the final redox equation is accurate.
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