Concentrate nitric acid oxidises phosphorus to phosphoric acid according to the following equation- P - 5HNO3conc- H3PO4 - H2O - 5NO2What mass of phosphoric acid can be prepared from 6-2 g of phosphorous-

P + 5HNO_3 → H_3PO_4 + H_2O + 5NO_2 No. of moles of P = #160; 9.331 = 0.3 moles. ...

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Standard X

Chemistry

Mole Concept

Concentrate n...

Question

Concentrate nitric acid oxidises phosphorus to phosphoric acid according to the following equation:
$P + 5 H N O_{3} (c o n c .) \to H_{3} P O_{4} + H_{2} O + 5 N O_{2}$
What mass of phosphoric acid can be prepared from $6.2 g$ of phosphorous?

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Solution

$P + 5 H N O_{3} \to H_{3} P O_{4} + H_{2} O + 5 N O_{2}$
No. of moles of P = $\frac{9.3}{31}$ = $0.3$ moles.

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Q. Concentrate nitric acid oxidises phosphorus to phosphoric acid according to the following equation:

P + 5 H N O_{3} (c o n c .) \to H_{3} P O_{4} + H_{2} O + 5 N O_{2}

9.3 g

of phosphorus was used in the reaction, calculate:
The mass of phosphoric acid formed.

Q. Concentrate nitric acid oxidises phosphorus to phosphoric acid according to the following equation:

P + 5 H N O_{3} (c o n c .) \to H_{3} P O_{4} + H_{2} O + 5 N O_{2}

9.3 g

of phosphorus was used in the reaction, calculate:
The volume of nitrogen dioxide produced at

S T P

[H = 1, N = 14, P = 31, O = 16]

Concentrated nitric acid oxidises phosphorus to phosphoric acid according to the following equation:
$P + 5 H N O_{3} \to H_{3} P O_{4} + 5 N O_{2} + H_{2} O$
If 6.2 g of phosphorus was used in the reaction, calculate:

(a) The number of moles of phosphorus taken and mass of phosphoric acid formed.
(b) Mass of nitric acid consumed at the same time.
(c) The volume of steam produced at the same time if measured at 760 mm Hg pressure and $273^{\circ} C .$

(a) Concentrated nitric acid oxidises phosphorus to phosphoric acid according to the following equation:
P + 5HNO₃ $\overset{}{\to}$ H₃PO₄ + H₂O + 5NO₂
(i) What mass of phosphoric acid can be prepared from 6.2 g of phosphorus?
(ii) What mass of nitric acid will be consumed at the same time?
(iii) 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)

(b) Ammonia may be oxidised to nitrogen monoxide in the presence of a catalyst according to the following equation:
4NH₃ + 5O₂ $\overset{}{\to}$ 4NO + 6H₂O
If 27 litres of reactants are consumed, what volume of nitrogen monoxide is produced at the same temperature and pressure?

P + 5 H N O_{3} \to H_{3} P O_{4} + H_{2} O + 5 N O_{2}

The mass of phosphoric acid that can be prepared from 6.2 g of phosphorous and the mass of

H N O_{3}

that will be consumed at the same time is respectively :

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Concentrate nitric acid oxidises phosphorus to phosphoric acid according to the following equation:P+5HNO3(conc.)→H3PO4+H2O+5NO2What mass of phosphoric acid can be prepared from 6.2 g of phosphorous?

P+5HNO3→H3PO4+H2O+5NO2No. of moles of P = 9.331 = 0.3 moles.

Concentrate nitric acid oxidises phosphorus to phosphoric acid according to the following equation:
$P + 5 H N O_{3} (c o n c .) \to H_{3} P O_{4} + H_{2} O + 5 N O_{2}$
What mass of phosphoric acid can be prepared from $6.2 g$ of phosphorous?

$P + 5 H N O_{3} \to H_{3} P O_{4} + H_{2} O + 5 N O_{2}$
No. of moles of P = $\frac{9.3}{31}$ = $0.3$ moles.