The reaction of $NO with N_{2} O_{4} at 250 K$ gives

$N_{2} O$

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${NO}_{2}$

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$N_{2} O_{5}$

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$N_{2} O_{3}$

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Solution

The correct option is D
$N_{2} O_{3}$

The explanation for the correct option:
D: $N_{2} O_{3}$
Nitric oxide reacts with dinitrogen tetroxide at $250 K$ to produce dinitrogen trioxide.
The following reaction takes place:
$2 NO (g) + N_{2} O_{4} (l) \overset{250 K}{\to} 2 N_{2} O_{3} (blue solid) Nitric Dinitrogen Dinitrogen oxide tetroxide trioxide$
Final Answer: Therefore, option D is the correct option.

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_{4}

_{3}

250^{\circ} - 260^{\circ} C

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