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Standard XII

Chemistry

Oxyacids of Phosphorus

Starting with...

Question

Starting with elemental phosphorus, $P_{4}$ , phosphoric acid can be prepared as shown
$P_{4} (s) + 5 O_{2} (g) ⟶ P_{4} O_{10} (s) H_{2} O ⟶ H_{3} P O_{4}$

True

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False

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Solution

The correct option is A True
Method of preparation of $H_{3} P O_{4}$
$P_{4} (s) + 5 O_{2} (g) ⟶ P_{4} O_{10} (s)$
$P_{4} O_{10} (s) + 6 H_{2} O ⟶ 4 H_{3} P O_{4}$
Hence, solid phosphorous is used to prepare Phosphoric acid.

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Similar questions

Q. Phosphoric acid

(H_{3} P O_{4})

is prepared in a two-step process:
(1)

P_{4} + 5 O_{2} \to P_{4} O_{10}

(2)

P_{4} O_{10} + 6 H_{2} O \to 4 H_{3} P O_{4}

In step (1),

62 g

of phosphorus is made to react with excess oxygen to form

P_{4} O_{10}

with 85 % yield. In step (2), the yield of

H_{3} P O_{4}

obtained is 90 %. Calculate the mass of

H_{3} P O_{4}

produced.

Q. Phosphoric acid (

H_{3} P O_{4}

) is prepared in a two-step process.

P_{4} + 5 O_{2} \to P_{4} O_{10}

P_{4} O_{10} + 6 H_{2} O \to 4 H_{3} P O_{4}

186 g of phosphorus is made to react with excess oxygen which forms

P_{4} O_{10}

that has a 60 % yield. In the second reaction, 80% yield of

H_{3} P O_{4}

is obtained. The mass of

H_{3} P O_{4}

produced is:
(Molar mass of phosphorous = 31 g/mol)

Q. Phosphoric acid

(H_{3} P O_{4})

is prepared in a two-step process:
(1)

P_{4} + 5 O_{2} \to P_{4} O_{10}

(2)

P_{4} O_{10} + 6 H_{2} O \to 4 H_{3} P O_{4}

In step (1),

62 g

of phosphorus is made to react with excess oxygen to form

P_{4} O_{10}

with 85 % yield. In step (2), the yield of

H_{3} P O_{4}

obtained is 90 %. Calculate the mass of

H_{3} P O_{4}

produced.

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. Phosphoric acid is prepared in a two-step process. Find the mass of

H_{3} P O_{4}

formed when 124 g of

P_{4}

reacts with an excess of oxygen and then treated with sufficient water.

P_{4} + O_{2} ⟶ P_{4} O_{10}

P_{4} O_{10} + H_{2} O ⟶ H_{3} P O_{4}

(Molar mass of P = 31 g/mol)

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Starting with elemental phosphorus, P4, phosphoric acid can be prepared as shownP4(s)+5O2(g)⟶P4O10(s)H2O⟶H3PO4

The correct option is A TrueMethod of preparation of H3PO4P4(s)+5O2(g)⟶P4O10(s)P4O10(s)+6H2O⟶4H3PO4Hence, solid phosphorous is used to prepare Phosphoric acid.

Starting with elemental phosphorus, $P_{4}$ , phosphoric acid can be prepared as shown
$P_{4} (s) + 5 O_{2} (g) ⟶ P_{4} O_{10} (s) H_{2} O ⟶ H_{3} P O_{4}$

The correct option is A True
Method of preparation of $H_{3} P O_{4}$
$P_{4} (s) + 5 O_{2} (g) ⟶ P_{4} O_{10} (s)$
$P_{4} O_{10} (s) + 6 H_{2} O ⟶ 4 H_{3} P O_{4}$
Hence, solid phosphorous is used to prepare Phosphoric acid.