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Ideal Gas Equation

The time take...

Question

The time taken in hours for $N H_{2} N O_{2}$ to decompose 99% is:

1.396

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13.96

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139.6

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0.1396

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Solution

The correct option is D 13.96
$N H_{2} N O_{2} (a q) \to N_{2} O (g) + H_{2}) (l)$

$k = \frac{0.693}{2.1} = 0.33 h r^{- 1}$

$t = \frac{2.303}{k} l o g \frac{1}{0.01}$

$= 13.96 h r$

1 mol of $N H_{2} N O_{2} = 1 m o l o f N_{2} O$
Moles of $N H_{2} N O_{2} = \frac{6.2}{6.2} = 0.1 m o l .$
Moles of $N H_{2} N O_{2}$ decomposed = 0.099
Volume of $N_{2} O$ produced = 22.4 L $\times$ 0.099 $\equiv$ 2.217 L

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