The reaction $ { P_4 + 3NaOH + 3H_2O \to 3NaH_2PO_2 + PH_3} $ is an example of
- disproportionation reaction
- neutralization reaction
- double decomposition reaction
- pyrolytic reaction
The Correct Option is A
Solution and Explanation
$ {P4 +3NaOH + 3H2O -> 3\,NaH2PO2 +PH3}$
Oxidation state of $P$ in $P_4 = 0$
Oxidation state of $P$ in $PH_3 = -3$
Oxidation state of $P$ in
$ {NaH_2PO_2 = + 1}$
so, $ {P^0_4 -> \overset{-3}{PH_3} +H2\overset{+1}{PO^{-}_2}}$
Hence, this reaction is an example of disproportionation reaction. It is a chemical reaction, typically a redox reaction, where a molecule is transformed into two or more dissimilar products.
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Concepts Used:
Balancing a redox reaction
The method that is based on the difference in oxidation number of oxidizing agent and the reducing agent is known as oxidation number. The half-reaction method entirely depends on the division of the redox reactions into oxidation half and reduction half. It entirely depends on the individual which method to choose and use.
Oxidation Number Method:
Like various other reactions, it is very important to write the correct compositions and formulas. A very important thing to keep in mind while writing oxidation-reduction reactions is to write the compositions and formulas of the substances and the products present in the chemical reaction in a very correct manner.
Half-Reaction Method:
In this procedure, we decouple the equation into two halves. After that, we balance both the parts of the reaction separately. Finally, we add them together to get a balanced equation.