In the reaction, 𝐏4+3 KOH+3 H2 O →3 KH2 PO2+PH3, phosphorous is: (a) Only oxidized (b) Oxidized

step 1 In the reaction, in the reaction which I am writing here, P4 plus 3koh plus 3h plus 3h2 will giv

In the reaction, 𝐏4+3 KOH+3 H2 O →3 KH2 PO2+PH3, phosphorous...

In the reaction,
$\mathbf{P}_{4}+3 \mathrm{KOH}+3 \mathrm{H}_{2} \mathrm{O} \rightarrow 3 \mathrm{KH}_{2} \mathrm{PO}_{2}+\mathrm{PH}_{3}$, phosphorous is:
(a) Only oxidized
(b) Oxidized as well as rduced
(c) Only reduced
(d) Neither oxidized nor reduced

Labs

Want to see this concept in action?

NEW

Explore this concept interactively to see how it behaves as you change inputs.

View Labs

Key Concepts

Redox Reactions

Redox reactions involve the transfer of electrons between species, where one species is oxidized (loses electrons) and the other is reduced (gains electrons). Understanding this concept is crucial for analyzing reactions where elements experience changes in their oxidation states, as it explains how and why the electron exchange leads to the transformation of reactants into products.

Oxidation Numbers

Oxidation numbers are a bookkeeping tool used to assign values to elements in chemical species, indicating their degree of oxidation. By determining the oxidation states in a reaction, one can identify which species are oxidized and which are reduced, helping in the overall analysis of electron transfer and redox processes.

Disproportionation Reaction

A disproportionation reaction is a specific type of redox reaction where a single element undergoes both oxidation and reduction simultaneously. In such reactions, the same element appears in two different oxidation states in the products, highlighting its simultaneous loss and gain of electrons during the transformation process.

Please give Ace some feedback