Assertion :The reaction, $P_{4} + 3 N a O H + 3 H_{2} O \to 3 N a H_{2} P O_{2} + P H_{3}$ , is a disproportionation reaction. Reason: In a disproportionation reaction, neither oxidation nor reduction takes place.

Both Assertion and Reason are correct and Reason is the correct explanation for Assertion

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Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion

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Assertion is correct but Reason is incorrect

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Assertion is incorrect but Reason is correct

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Solution

The correct option is C Assertion is correct but Reason is incorrect

$_{4} + 3 N a O H + 3 H_{2} O \to - 3 P H_{3} + 3 N a H_{2} + 1 P O_{2}$

In the reaction between phosphorus and $N a O H$ , the oxidation state of phosphorus changes from $0$ to $- 3$ and $+ 1$ . The oxidation state of other atoms remains the same. Thus, phosphorus undergoes disproportionation reaction. In the disproportionation reaction, same substance is oxidized and reduced.

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Assertion :The reaction, P4+3NaOH+3H2O→3NaH2PO2+PH3, is a disproportionation reaction. Reason: In a disproportionation reaction, neither oxidation nor reduction takes place.

Assertion :The reaction, $P_{4} + 3 N a O H + 3 H_{2} O \to 3 N a H_{2} P O_{2} + P H_{3}$ , is a disproportionation reaction. Reason: In a disproportionation reaction, neither oxidation nor reduction takes place.