The half time of first order decomposition of nitramide is 2.1 hour at 15°C.
${NH}_{2} {NO}_{2} (aq .) \overset{}{\to} N_{2} O (g) + H_{2} O (l)$
If 6.2 g of $N H_{2} N O_{2}$ is allowed to decompose, calculate time taken in hours for $N H_{2} N O_{2}$ to decompose 99%. $[\log_{10} 2 = 0.3]$

Question

The half time of first order decomposition of nitramide is 2.1 hour at 15°C.

${NH}_{2} {NO}_{2} (aq .) \overset{}{\to} N_{2} O (g) + H_{2} O (l)$

If 6.2 g of $N H_{2} N O_{2}$ is allowed to decompose, calculate time taken in hours for $N H_{2} N O_{2}$ to decompose 99%. $[\log_{10} 2 = 0.3]$

Infinity Learn · Accepted Answer

∵ $$t=2.303klog10a(a$$−$$x)$$ If $$t=t2$$,$$x=a2$$;  ∴$$t1/2=2.303klog10aa-a2$$ . . . . . (1)If$$ $$t=t99$$%,  $$x=99a100$$;  $$t99$$%$$=2.303klog10aa$$−$$99a100$$ . . . . $$(2)By$$ Eqs. $$(1) and (2),$$t99$$%$$=log10100log102$$×$$t1/2=20.3010$$×$$2.1$$  $$=$$  $$13.95$$ hour

Kinetics of chemical reactions

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The half time of first order decomposition of nitramide is 2.1 hour at 15°C.
${NH}_{2} {NO}_{2} (aq .) \overset{}{\to} N_{2} O (g) + H_{2} O (l)$
If 6.2 g of $N H_{2} N O_{2}$ is allowed to decompose, calculate time taken in hours for $N H_{2} N O_{2}$ to decompose 99%. $[\log_{10} 2 = 0.3]$

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Kinetics of chemical reactions

Unlock the full solution & master the concept.

The half time of first order decomposition of nitramide is 2.1 hour at 15°C.NH2NO2(aq.)→ N2O(g)+H2O(l)If 6.2 g of NH2NO2 is allowed to decompose, calculate time taken in hours for NH2NO2 to decompose 99%.[log102=0.3]

∵ t=2.303klog10a(a−x) If t=t2,x=a2; ∴t1/2=2.303klog10aa-a2 . . . . . (1)If t=t99%, x=99a100; t99%=2.303klog10aa−99a100 . . . . (2)By Eqs. (1) and (2),t99%=log10100log102×t1/2=20.3010×2.1 = 13.95 hour

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The half time of first order decomposition of nitramide is 2.1 hour at 15°C.
${NH}_{2} {NO}_{2} (aq .) \overset{}{\to} N_{2} O (g) + H_{2} O (l)$
If 6.2 g of $N H_{2} N O_{2}$ is allowed to decompose, calculate time taken in hours for $N H_{2} N O_{2}$ to decompose 99%. $[\log_{10} 2 = 0.3]$