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

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 :

29.6 g, 63 g

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63 g, 63 g

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19.6 g, 63 g

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34 g, 19.4 g

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Solution

The correct option is D $19.6 g, 63 g$
Atomic weight of $P = 31 g$

Atomic weight of $H_{3} P O_{4} = 98 g$

We know that $31 g$ of $P$ will give 98 g of $H_{3} P O_{4}$ .

Therefore, $6.2 g$ of $P$ will give:= $\frac{98}{31} \times 6.2 = 19.6 g o f H_{3} P O_{4}$ .

Atomic weight of $P = 31 g$

Atomic weight of $5$ moles of $H N O_{3} = 315 g$ .

We know that $31 g$ of $P$ will give 315 g of $H N O_{3}$ .

Therefore, $6.2 g$ of $P$ will give: $\frac{315}{31} \times 6.2 = 63 g$ of $H N O_{3}$ .

Hence, option C is correct.

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Similar questions

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}

What mass of phosphoric acid can be prepared from

6.2 g

of phosphorous?

Q. A

10

% solution of

H N O_{3}

would be produced by dissolving

63 g

H N O_{3}

in how many

m L

water?

Q. What will be the volume of

N / 10

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63 g

of hydrated oxalic acid?

(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?

9.3 g of phosphorous was used in the reaction shown.

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

Calculate the number of moles of phosphorus taken.

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P+5HNO3→H3PO4+H2O+5NO2The mass of phosphoric acid that can be prepared from 6.2 g of phosphorous and the mass of HNO3 that will be consumed at the same time is respectively :

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

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 :