The half life of first order decomposition of nitramide is 2-1 hours at 15- C-NH2NO2aq- N2Og-H2OlCalculate time taken for 99

K=0.693t_1/2=0.6932.1=0.33 hrs^ 1 Applying kinetic equations of first order reaction, k=2.303tlog_10a(a x) nbsp; nbsp; nbsp; nbsp; t=2.3030.33log_1 ...

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Standard XII

Chemistry

Molarity

The half life...

Question

The half life of first order decomposition of nitramide is 2.1 hours at $15^{\circ} C .$
$N H_{2} N O_{2} (a q .) \to N_{2} O (g) + H_{2} O (l)$

Calculate time taken for 99% decomposition of $N H_{2} N O_{2}$

13.96 h r

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44.43 h r

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28.23 h r

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None of the above

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Solution

The correct option is A $13.96 h r$
$k = \frac{0.693}{t_{1 / 2}} = \frac{0.693}{2.1} = 0.33 h r s^{- 1}$
Applying kinetic equations of first order reaction,
$k = \frac{2.303}{t} l o g_{10} \frac{a}{(a - x)}$

$t = \frac{2.303}{0.33} l o g_{10} \frac{100}{(100 - 99)}$
$t = 13.96 h r$

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The half life of first order decomposition of nitramide is 2.1 hours at 15∘C. NH2NO2(aq.)→N2O(g)+H2O(l) Calculate time taken for 99% decomposition of NH2NO2

The correct option is A 13.96 hrk=0.693t1/2=0.6932.1=0.33 hrs−1 Applying kinetic equations of first order reaction, k=2.303tlog10a(a−x) t=2.3030.33log10100(100−99) t=13.96 hr

The half life of first order decomposition of nitramide is 2.1 hours at $15^{\circ} C .$
$N H_{2} N O_{2} (a q .) \to N_{2} O (g) + H_{2} O (l)$

Calculate time taken for 99% decomposition of $N H_{2} N O_{2}$

The correct option is A $13.96 h r$
$k = \frac{0.693}{t_{1 / 2}} = \frac{0.693}{2.1} = 0.33 h r s^{- 1}$
Applying kinetic equations of first order reaction,
$k = \frac{2.303}{t} l o g_{10} \frac{a}{(a - x)}$

$t = \frac{2.303}{0.33} l o g_{10} \frac{100}{(100 - 99)}$
$t = 13.96 h r$