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Question

Concentrated nitric acid oxidizes phosphorus to phosphoric acid according to the following equations :

P+5HNO3CONC.H3PO4+H2O+5NO2

If 9.3g of phosphorus was used in the reactions, calculate: The volume of nitrogen dioxide produced at STP.


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Solution

Step-1. Given reaction :

P(s)+5HNO3(conc.)(L)H3PO4(s)+H2O(L)+5NO2(g)(Phosphorus)(Nitricacid)(Phosphoric(water)(nitrogenacid)dioxide)

From the given reaction, it is concluded that 5 moles of NO2 are formed during the reaction.

Step-2. The volume of 1 mole of NO2 at STP =22.4×5

=112.0L

Step-3. If 31g of phosphorus released 112.0L of NO2 at STP

Then 9.3g of Phosphorus releases =11231×9.3

=33.6L

Hence, 9.3gof Phosphorus releases 33.6L of nitrogen dioxide.


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