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Metal Oxide and Hydroxide

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the following data are for the decomposition of ammonium nitrate in aqueous solution volume of N2 in cc time in min 6.25 10 9.50 15 11.42 20 13.65 25 35.05 finally the order of the reaction is 1)zero 2)one 3)two 4)t

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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. 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. The decomposition of an aqueous solution of ammonium nitrite was studied. The volume of nitrogen gas collected at different intervals of time was follows:

\begin{matrix} T i m e (m i n u t e s) & 10 & 15 & 20 & \infty V o l . o f N_{2} (m L) & 6.25 & 9.00 & 11.40 & 35.05 \end{matrix}

From the above data prove that the reaction is of the first order.

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.

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