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Oxides of Nitrogen

Which oxide o...

Question

Which oxide of nitrogen is the most stable:

A

2NO_2(g) N_2(g) + 2O_2(g); K = 6.7 x 10¹⁶mollitre^-1

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B

2NO_(g) N_2(g) + O_2(g); K = 2.2 x 10³⁰mol litre^-1

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C

2N₂O_5(g) 2N_2(g) + 5O_2(g); K = 1.2 x 10³⁴ mol^-5 litre^-5

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D

2N₂O_(g) 2N_2(g) + O_2(g); K = 3.5 x 10³³mol litre^-1

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Solution

The correct option is A
2NO_2(g) N_2(g) + 2O_2(g); K = 6.7 x 10¹⁶mollitre^-1

Lesser the K value , higher is the stability of oxide.

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Similar questions

Reaction	$K$
$\frac{1}{2} N_{2} (g) + O_{2} (g) ⇋ N O_{2}$	$K_{1}$
$2 N O_{2} (g) ⇌ N_{2} O_{4} (g)$	$K_{2}$

Using the above equations, write down expression for

K

of the following reaction:

N_{2} O_{4} (g) ⇌ N_{2} (g) + \frac{1}{2} O_{2} (g)

Q. If the equilibrium constant for

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

K

, the equilibrium constant for

\frac{1}{2} N_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ N O (g)

Q. If the equilibrium constant for

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

K

, the equilibrium constant for

\frac{1}{2} N_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ N O (g)

Q. The equilibrium constant for the reactions

N_{2 (g)} + O_{2_{(} g)} ⇋ 2 N O_{(g)}

N O_{(g)} ⇋ \frac{1}{2} N_{2 (g)} + \frac{1}{2} O_{2_{(} g)}

k^{1}

, the relation between k and

k^{1}

Q. The equilibrium constant for the reactions are

K

K^{1}

respectively, the relation between

K

K^{1}

N_{2_{(g)}} + O_{2_{(g)}} ⇆ 2 {N O}_{(g)}

{N O}_{(g)} ⇌ \frac{1}{2} N_{2_{(g)}} + \frac{1}{2} O_{2_{(g)}}

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