In the following rection 4 P+3 KOH+3 H2 O ⟶3 KH2 PO2+PH3 (a) P is only oxidized (b) P is only re

step 1 So in this question they ask the tense. In the following reaction 4p plus 3kosh plus 3 h2 h22 pl

In the following rection 4 P+3 KOH+3 H2 O ⟶3 KH2 PO2+PH3 (a)...

In the following rection

$$
4 \mathrm{P}+3 \mathrm{KOH}+3 \mathrm{H}_2 \mathrm{O} \longrightarrow 3 \mathrm{KH}_2 \mathrm{PO}_2+\mathrm{PH}_3
$$

(a) P is only oxidized
(b) P is only reduced
(c) P is both oxidized as well as reduced
(d) none of these

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Key Concepts

Disproportionation Reaction

A disproportionation reaction is a specific type of redox reaction in which a single element undergoes both oxidation and reduction simultaneously. This means that the same element is transformed into two different oxidation states – one higher and one lower than its original state – which is central to understanding the behavior of substances like phosphorus in certain reactions.

Oxidation States

Oxidation states are numerical values assigned to atoms in a compound in order to indicate the degree of oxidation (loss of electrons) of an atom. These states are used to keep track of electron shifts during chemical processes, and they are key in determining whether a substance is oxidized or reduced in a reaction.

Oxidation-Reduction Reactions

These are chemical reactions in which the oxidation states of atoms are changed. Typically, one reactant loses electrons (is oxidized) while another gains electrons (is reduced), and the overall process involves the transfer of electrons between species. This concept is crucial for understanding how the distribution of electrons changes during a reaction.

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