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Hydrogenation of Alkynes

Which of the ...

Question

Which of the following is correct about the product obtained when equimolar amount of $N O$ and $N O_{2}$ are condensed together?

A

It is an acidic oxide and can be dissolved in alkalies to give nitrites

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B

It is referred to as the anhydride of nitrous acid

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C

It has both symmetrical and asymmetrical forms

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D

All of these

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Solution

The correct option is D All of these
$N O + N O_{2} ⟶ N_{2} O_{3}$

(a) $N_{2} O_{3}$ is the anhydride of nitrous acid.

(b) $N_{2} O_{3}$ on reaction with alkali forms nitrites.
$N_{2} O_{3} + 2 K O H \to 2 K N O_{2} + H_{2} O$
$N_{2} O_{3} + 2 N a O H \to 2 N a N O_{2} + H_{2} O$

(c) $N_{2} O_{3}$ exists in two different forms:

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Similar questions

Q. Which of the following is correct about the product obtained when equimolar amount of

N O

N O_{2}

are condensed together?

Q. Which of the following represents the products obtained when

N a O H

N O_{2}

?

N O

N O_{2}

are mixed, the following equilibria are readily obtained :

2 N O_{2} ⇌ N_{2} O_{4} K_{p} = 6.8 a t m^{- 1}

N O + N O_{2} ⇌ N_{2} O_{3}

In an experiment when

N O

N O_{2}

are mixed in the ratio of

1 : 2

, the final total pressure was

5.05 a t m

and the partial pressure of

N_{2} O_{4}

1.7 a t m

. Calculate the equilibrium partial pressure of

N O

in atmosphere :

N O

N O_{2}

are mixed, the following equilibria are readily obtained;

2 N O_{2} ⇌ N_{2} O_{4}, K_{P} = 6.8 a t m^{- 1} a n d N O + N O_{2} ⇌ N_{2} O_{3}

In an experiment when

N O

N O_{2}

are mixed in the ratio of 1 : 2, the find total pressure was 5.05 atm and the partial pressure of

N_{2} O_{4}

was 1.7 atm. Calculate the equilibrium partial pressure of NO in atmosphere.

N O

N O_{2}

are mixed, the following equilibria are readily obtained :

2 N O_{2} ⇌ N_{2} O_{4} K_{p} = 6.8 a t m^{- 1}

N O + N O_{2} ⇌ N_{2} O_{3}

In an experiment when

N O

N O_{2}

are mixed in the ratio of

1 : 2

, the final total pressure was

5.05 a t m

and the partial pressure of

N_{2} O_{4}

1.7 a t m

. Calculate the equilibrium partial pressure of

N O

in atmosphere :

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