$0.44 g$ of a colourless oxide of nitrogen occupies $224 m L$ at STP. The compound is

N_{2} O

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N O

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N_{2} O_{2}

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N O_{2}

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Solution

The correct option is A $N_{2} O$
$1 m o l e$ of any substance occupies $22400 m l$
So,
$224 m l$ of substance has $0.44 g$ mass $22400 m l$
$\frac{0.44}{224} \times 22400$
$\Rightarrow 44 g$
Molecular mass
$N_{2} O = 14 \times 2 + 16$
$= 44 g$ .

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When $0.44 g$ of a colourless oxide of nitrogen occupies $224 m L$ at $1520 m m$ of $H g$ and $273^{\circ}C$ , then the oxide is

0.44 g

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When 0.44g of colourless oxide of nitrogen occupies 224 mL at 1520 mm of HG and 273 degree Celsius , then the oxide is ???

N O, N O_{2}, N_{2} O, N_{2} O_{4}

N_{2} O_{2}

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