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प्रश्न
Concentrated nitric acid oxidises phosphorus to phosphoric acid according to the following equation:
\[\ce{P + 5HNO3 -> H3PO4 + H2O + 5NO2}\]
- What mass of phosphoric acid can be prepared from 6.2 g of phosphorus?
- What mass of nitric acid will be consumed at the same time?
- What will be the volume of steam at the same time measured at 760 mm Hg pressure and 373°C?
(H = 1; N = 14; O = 16; P = 31∴ )
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उत्तर
\[\ce{\underset{31 g}{P} + 5HNO3 -> \underset{(98 g)}{H3PO4} + H2O + 5NO2}\]
i. 31 g of P = 1 mole
∴ 9.3 g of P = `1/31 xx 9.3`
= 0.3 moles
Hence, 0.3 moles of phosphorus were taken for the reaction.
ii. 31 g of P forms 98 g of phosphoric acid.
∴ 9.3 g of P = `98/31 xx 9.3`
= 29.4 g
Hence, 29.4 g of phosphoric acid is formed.
iii. 31 g of P produces 5 vol = 5 × 22.4 lit.
∴ 9.3 g will produce = `(5 xx 22.4)/31`
= 33.6 lit.
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