Choose the correct on from the given four options-Consider equation- P4O10 - H2O - H3PO4- Number of moles of H3PO4 produced by reaction are 1 mole of P4O10 is -

#160;The balanced equation is : P4O10 #160;+ 6H2O #8594; 4H3PO44 moles of #160; #160;H3PO4 will be formed from 1 mol of P_4O_10 So, 2^nd ...

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Byju's Answer

Standard XII

Chemistry

Preparation of Carboxylic Acids

Choose the co...

Question

Choose the correct on from the given four options:
Consider equation:
P₄O₁₀ + H₂O → H₃PO₄.
Number of moles of H₃PO₄ produced by reaction are 1 mole of $P_{4} O_{10}$ is _________.
2
4
6
8

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Solution

The balanced equation is : P₄O₁₀ + 6H₂O → 4H₃PO₄
_{4 moles of}H₃PO_{4 will be formed from 1 mol of $P_{4} O_{10}$}
_{So, $2^{n d}$ option is correct.}

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Similar questions

Q. Phosphoric acid

(H_{3} {PO}_{4})

prepared in a two step process.
(1)

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

(2)

P_{4} O_{10} + {6H}_{2} O \to {4H}_{3} {PO}_{4}

We allow 62 g of phosphorus to react with excess oxygen which form

P_{4} O_{10}

which gives 85% yield. If in the step (2) reaction, 90% yield of

H_{3} {PO}_{4}

is obtained then mass of

H_{3} {PO}_{4}

produced is:

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. Consider reaction:

P_{4} O_{10} (s) + H_{2} O (l) ⟶ H_{3} P O_{4} (a q)

Moles of

H_{2} O

required to balance equation will be:

Q. Phosphoric acid (

H_{3} P O_{4}

) is widely used to make fertilizers and can be prepared in a two-step process.

S t e p I : P_{4} + 5 O_{2} ⟶ P_{4} O_{10}

S t e p I I : P_{4} O_{10} + 6 H_{2} O ⟶ 4 H_{3} P O_{4}

We allow

310

g of phosphorus to react with excess oxygen, which forms tetraphosphorus deoxide (

P_{4} O_{10}

) in

50 %

yield. In the step

I I

25 %

yield of

H_{3} P O_{4}

is obtained.
(Atomic weight in amu of

P = 31, H = 1, O = 16

)

Assuming

100 %

yield, the number of moles of

H_{3} P O_{4}

is :

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.

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Choose the correct on from the given four options:Consider equation: P4O10 + H2O → H3PO4. Number of moles of H3PO4 produced by reaction are 1 mole of P4O10 is _________.2468

The balanced equation is : P4O10 + 6H2O → 4H3PO44 moles of H3PO4 will be formed from 1 mol of P4O10So, 2nd option is correct.

Choose the correct on from the given four options:
Consider equation:
P₄O₁₀ + H₂O → H₃PO₄.
Number of moles of H₃PO₄ produced by reaction are 1 mole of $P_{4} O_{10}$ is _________.
2
4
6
8

The balanced equation is : P₄O₁₀ + 6H₂O → 4H₃PO₄
_{4 moles of}H₃PO_{4 will be formed from 1 mol of $P_{4} O_{10}$}
_{So, $2^{n d}$ option is correct.}