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Decomposition Reaction

13. Calculate...

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13. Calculate the rate constant for decomposition of ammonium nitrate from the following data NH4NO2 ---> N2 + 2H2O Time(minutes) : 10, 25, infinity Vol. Of N2 (ml) : 6.25, 13.65, 35.05

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Q. Calculate the rate constant for decomposition of ammonium nitrite from the following.

Time (minutes)	$10$	$20$	$\infty$
Vol. of $N_{2}$ (ml)	$6.25$	$13.65$	$35.05$

N H_{4} N O_{2} \to N_{2} + 2 H_{2} O

[Given that the reaction follows first order kinetics]

Q. Calculate the rate constant for decomposition of ammonium nitrate from the following data;

N H_{4} N O_{2} \to N_{2} + 2 H_{2} O

Time (minutes)	10	25	$\infty$
Vol.of $N_{2}$ ml	6.25	13.65	35.05

Given that the reaction follows first order kinectics.

Volume of $N_{2}$ (in cc)	Time (in minutes)
6.25	10
9	15
11.4	20
13.65	25
35.05	$\infty$

The following data is for the decomposition of ammonium nitrite in aqueous solution.

The order of the reaction is:

Q. The following data are for the decomposition of ammonium nitrate in aqueous solution:

\begin{matrix} V o l u m e o f N_{2} (c m^{3}) & 6.25 & 9.0 & 11.42 & 13.65 & 35.02 T i m e (m i n) & 10 & 15 & 20 & 25 & \infty \end{matrix}

The order of reaction is:

Q. The following data represents for the decomposition of

N H_{4} N O_{2}

is an aqueous solution:

Time in min	10	15	20	25	$\infty$
Volume of $N_{2}$ (in mL)	6.25	9.0	11.40	13.64	33.05

Velocity constant is:

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