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Standard IX

Chemistry

Mole Concept

9.3 g of phos...

Question

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.

1.5

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0.3

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2.5

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Solution

The correct option is A 0.3
Given that
Mass of P used, w = 9.3 g
Molar mass of P, M = 31 g/mol

Now
Moles of phosphorous = $\frac{w}{M} = \frac{9.3}{31} = 0.3$ mol

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Similar questions

9.3 g of phosphorous was taken in the reaction shown:

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

Calculate the volume of

N O_{2}

produced at S.T.P..

[

H

= 1,

N

= 14,

P

= 31,

O

= 16]

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.

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 $273^{\circ} C .$

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

What would be the volume of steam produced from 6.2 g of phosphorus at

S T P

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

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]

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9.3 g of phosphorous was used in the reaction shown. P+5HNO3⟶H3PO4+H2O+5NO2Calculate the number of moles of phosphorus taken.

The correct option is A 0.3Given thatMass of P used, w = 9.3 gMolar mass of P, M = 31 g/molNowMoles of phosphorous = wM=9.331=0.3 mol

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.

The correct option is A 0.3
Given that
Mass of P used, w = 9.3 g
Molar mass of P, M = 31 g/mol

Now
Moles of phosphorous = $\frac{w}{M} = \frac{9.3}{31} = 0.3$ mol