Answer
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Hint: Start this question by writing the complete equation and balance it. Also, keep in mind the oxidation states and atomic numbers while solving it.
Complete step by step answer:
The reaction given above is an example of disproportionation reaction. It is because \[{{P}_{4}}\]acts both as an oxidant and reductant.
White phosphorus reacts with a cold and concentrated solution of sodium hydroxide and water to produce phosphine and sodium hypophosphite. This reaction takes place slowly.
We can balance the given equation as –
\[{{P}_{4}}+3NaOH+3{{H}_{2}}O\to P{{H}_{3}}+3Na{{H}_{2}}P{{O}_{2}}\]
From the reaction we can see that there are 3 moles of \[Na{{H}_{2}}P{{O}_{2}}\] (sodium hypophosphite) and 1 mole of \[P{{H}_{3}}\].
Therefore, the answer is – the mole ratio of \[Na{{H}_{2}}P{{O}_{2}}\] and \[P{{H}_{3}}\]in the given reaction is 3.
Additional information:
Reactants –
White phosphorus - \[{{P}_{4}}\]
White phosphorus or simply tetraphosphorus (\[{{P}_{4}}\]) exists as molecules which is made up of four atoms in a tetrahedral structure. The tetrahedral arrangement results in ring strain and instability.
Sodium hydroxide - \[NaOH\]
Water - \[{{H}_{2}}O\]
Products –
Phosphine - \[P{{H}_{3}}\]
It is a colorless, flammable, toxic gas and is classified as a pnictogen hydride. Phosphine burns and produces a dense white cloud of phosphoric acid.
Sodium hypophosphite - \[Na{{H}_{2}}P{{O}_{2}}\]
Sodium hypophosphite is also known as sodium phosphinate. It is the sodium salt of hypophosphorous acid. It is a solid at room temperature and appears as odorless white crystals.
Note: The given reaction is a disproportionation reaction. It is also known as redox reaction in which a compound of intermediate oxidation state converts to two different compounds, one of higher and one of lower oxidation states, and hence oxidation and reduction takes place simultaneously.
Complete step by step answer:
The reaction given above is an example of disproportionation reaction. It is because \[{{P}_{4}}\]acts both as an oxidant and reductant.
White phosphorus reacts with a cold and concentrated solution of sodium hydroxide and water to produce phosphine and sodium hypophosphite. This reaction takes place slowly.
We can balance the given equation as –
\[{{P}_{4}}+3NaOH+3{{H}_{2}}O\to P{{H}_{3}}+3Na{{H}_{2}}P{{O}_{2}}\]
From the reaction we can see that there are 3 moles of \[Na{{H}_{2}}P{{O}_{2}}\] (sodium hypophosphite) and 1 mole of \[P{{H}_{3}}\].
Therefore, the answer is – the mole ratio of \[Na{{H}_{2}}P{{O}_{2}}\] and \[P{{H}_{3}}\]in the given reaction is 3.
Additional information:
Reactants –
White phosphorus - \[{{P}_{4}}\]
White phosphorus or simply tetraphosphorus (\[{{P}_{4}}\]) exists as molecules which is made up of four atoms in a tetrahedral structure. The tetrahedral arrangement results in ring strain and instability.
Sodium hydroxide - \[NaOH\]
Water - \[{{H}_{2}}O\]
Products –
Phosphine - \[P{{H}_{3}}\]
It is a colorless, flammable, toxic gas and is classified as a pnictogen hydride. Phosphine burns and produces a dense white cloud of phosphoric acid.
Sodium hypophosphite - \[Na{{H}_{2}}P{{O}_{2}}\]
Sodium hypophosphite is also known as sodium phosphinate. It is the sodium salt of hypophosphorous acid. It is a solid at room temperature and appears as odorless white crystals.
Note: The given reaction is a disproportionation reaction. It is also known as redox reaction in which a compound of intermediate oxidation state converts to two different compounds, one of higher and one of lower oxidation states, and hence oxidation and reduction takes place simultaneously.
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