Question detail
When balancing the redox equation for the reaction between hydrogen peroxide and iodide ions, what is the oxidation state of iodine in the product?
Try the question, check the answer, then read the explanation to understand the curriculum point.
At a glance
MCQ
Type
practice
Style
Topic
Oxidation, reduction and redox equations
Question
- A. -1
- B. 0
- C. +1
- D. +5
Answer
The oxidation state of iodine in the product is +1.
Explanation
In the reaction, iodide ions (I-) are oxidized to iodine (I2), which has an oxidation state of 0. However, in the presence of hydrogen peroxide, iodine can be oxidized further to +1 in the product. This reflects the increase in oxidation state, confirming iodine's role as a reducing agent.
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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