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Sigma Bond and Pi Bond

Identify oxid...

Question

Identify oxidant and reductant in the following redox reactions.
$P_{4} + 5 O_{2} ⟶ P_{4} O_{10}$

A

Oxidant:

O_{2}

; Reductant:

P_{4} O_{10}

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B

Oxidant:

P_{4}

; Reductant:

O_{2}

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C

Oxidant:

O_{2}

; Reductant:

P_{4}

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D

None of these

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Solution

The correct option is C Oxidant: $O_{2}$ ; Reductant: $P_{4}$
The balanced redox reaction is $P_{4} + 5 O_{2} ⟶ P_{4} O_{10}$ .
The oxidation number of oxygen changes from 0 to -2. Thus, oxygen is reduced.
The oxidant is $O_{2}$ .
The oxidation number of P changes from 0 to +5. Thus, P is oxidized.
The reductant is $P_{4}$ .

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Q. Two substance,

P_{4}

O_{2}

are allowed to react completely to form mixture of

P_{4} O_{6}

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leaving none of the reactants. The composition of final mixture if

P_{4}

O_{2}

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P_{4} + 5 O_{2} \to P_{4} O_{10}

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P_{4}

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O_{2}

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P_{4}

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O_{2}

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