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In the reaction 2K(3)[Fe(CN)(6)] + 2KO...

In the reaction
`2K_(3)[Fe(CN)_(6)] + 2KOH + H_(2)O_(2)rarr`
`2K_(4)[Fe(CN)_(6)] + 2H_(2)O + O_(2)`
`H_(2)O_(2)` acts as

A

Reducing agent

B

Oxidising agent

C

Knocking agent

D

Bleaching agent

Text Solution

AI Generated Solution

The correct Answer is:
To determine the role of hydrogen peroxide (H₂O₂) in the given reaction, we need to analyze the oxidation states of the elements involved, particularly iron (Fe). ### Step-by-Step Solution: 1. **Write the Reaction**: The reaction given is: \[ 2K_3[Fe(CN)_6] + 2KOH + H_2O_2 \rightarrow 2K_4[Fe(CN)_6] + 2H_2O + O_2 \] 2. **Determine Oxidation States**: - **For the reactant** \( K_3[Fe(CN)_6] \): - Let the oxidation state of Fe be \( x \). - The oxidation state of K is +1 (3 K atoms contribute +3). - The oxidation state of CN is -1 (6 CN groups contribute -6). - Setting up the equation: \[ 3(+1) + x + 6(-1) = 0 \implies 3 + x - 6 = 0 \implies x = +3 \] - Thus, the oxidation state of Fe in \( K_3[Fe(CN)_6] \) is +3. - **For the product** \( K_4[Fe(CN)_6] \): - Let the oxidation state of Fe be \( y \). - The oxidation state of K is +1 (4 K atoms contribute +4). - The oxidation state of CN is -1 (6 CN groups contribute -6). - Setting up the equation: \[ 4(+1) + y + 6(-1) = 0 \implies 4 + y - 6 = 0 \implies y = +2 \] - Thus, the oxidation state of Fe in \( K_4[Fe(CN)_6] \) is +2. 3. **Analyze the Change in Oxidation State**: - In the reaction, Fe changes from +3 to +2. This indicates that Fe is being reduced (gaining electrons). 4. **Identify the Role of H₂O₂**: - Since H₂O₂ is facilitating the reduction of Fe from +3 to +2, it is acting as a reducing agent in this reaction. 5. **Conclusion**: - Therefore, in this reaction, hydrogen peroxide (H₂O₂) acts as a **reducing agent**.
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