$P_{4} + 3 N a O H + 3 H_{2} O ⟶ 3 N a (H_{2} P O_{2}) + P H_{3}$ is an example of:

Disproportionation reaction

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Neutralisation reaction

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Double decomposition reaction

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Pyrolytic reaction

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Solution

The correct option is A
Disproportionation reaction

${0 P}_{4} + 3 N a O H + 3 H_{2} O ⟶ 3 N a (H_{2} + 1 P O_{2}) + - 3 P H_{3}$

Clearly, this is a disproportionation reaction. On the left hand side, elemental Phosphorus has oxidation state 0. In $P H_{3}$ oxidation state of Phosphorus is -3. In Sodium hypophosphite, the oxidation state of Phosphorus is +1.

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Similar questions

P_{4} + 3 N a O H + 3 H_{2} O \to 3 N a H_{2} P O_{2} + P H_{3}

P_{4} + 3 N a O H + 3 H_{2} O ⟶ 3 N a (H_{2} P O_{2}) + P H_{3}

P_{4} + 3 N a O H + 3 H_{2} O ⟶ 3 N a (H_{2} P O_{2}) + P H_{3}

$P_{4} + 3 N a O H + 3 H_{2} O ⟶ 3 N a (H_{2} P O_{2}) + P H_{3}$ is an example of:

P_{4} + 3 N a O H + 3 H_{2} O \to

3 N a H_{2} P O_{2} + P H_{3}

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