Which of the following reaction is an example of a redox reaction ?

X e F_{2} + P F_{5} \to [X e F]^{+} + {P F_{6}}^{-}

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X e F_{6} + H_{2} O \to X e O F_{4} + 2 H F

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X e F_{6} + 2 H_{2} O \to X e O_{2} F_{2} + 4 H F

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X e F_{4} + O_{2} F_{2} \to X e F_{6} + O_{2}

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Solution

The correct option is D $X e F_{4} + O_{2} F_{2} \to X e F_{6} + O_{2}$
The reaction $X e F_{4} + O_{2} F_{2} \to X e F_{6} + O_{2}$ is an example of a redox reaction.

The oxidation number of $X e$ increases from $+ 4 (X e F_{4})$ to $+ 6 (X e F_{6})$ . Hence, it is oxidised.

The oxidation number of oxygen decreases from $+ 1 (O_{2} F_{2})$ to $0 (O_{2})$ . Hence, it is reduced.

Hence, the option (D) is the correct answer.

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Similar questions

X e F_{6} + H_{2} O ⇌ X e O F_{4} + 2 H F

= k_{1}, X e O_{4} + X e F_{6} ⇌ X e O F_{4} + X e O_{3} F_{2}

= K_{2}

X e O_{4} + 2 H F ⇌ X e O_{3} F_{2} + H_{2} O

X e F_{6} + H_{2} O ⇌ X e O F_{4} + 2 H F

= K_{1}, X e O_{4} + X e F_{6} ⇌ X e O F_{4} + X e O_{3} F_{2}

= K_{2}

- X e O_{4} + 2 H F ⇌ X e O_{4} F_{2} + H_{2} O

X e F_{4} + O_{2} F_{2} \to

X e F_{6} + O_{2}

X e O_{2} F_{2}, X e O F_{4}, X e F_{4}, X e F_{6}

X e

X e F_{6} + H_{2} O

\to

+ 2 H F

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