The decomposition of nitramide in aqueous solution at 25 °C NH;NO;(aq) N3O(e) + H;O() is first order in NH,NO; with a rate constant of 4.1 4.70-10 s-!. If the initial concentration of NH2NO, is 0.848 M, the concentration of NH2NO, will be Mafter 28016 s have passed.

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**The Decomposition of Nitramide in Aqueous Solution at 25 °C**

The reaction for the decomposition of nitramide is given by:

\[ \text{NH}_2\text{NO}_2(\text{aq}) \rightarrow \text{N}_2\text{O}(\text{g}) + \text{H}_2\text{O}(\ell) \]

This reaction is first order in \(\text{NH}_2\text{NO}_2\) with a rate constant of \(4.70 \times 10^{-5} \, \text{s}^{-1}\).

**Problem:**

If the initial concentration of \(\text{NH}_2\text{NO}_2\) is 0.848 M, calculate the concentration of \(\text{NH}_2\text{NO}_2\) after 28,016 seconds.

Solution: \[ \_\_\_\_\_ \text{M} \] After 28,016 seconds have passed.
Transcribed Image Text:**The Decomposition of Nitramide in Aqueous Solution at 25 °C** The reaction for the decomposition of nitramide is given by: \[ \text{NH}_2\text{NO}_2(\text{aq}) \rightarrow \text{N}_2\text{O}(\text{g}) + \text{H}_2\text{O}(\ell) \] This reaction is first order in \(\text{NH}_2\text{NO}_2\) with a rate constant of \(4.70 \times 10^{-5} \, \text{s}^{-1}\). **Problem:** If the initial concentration of \(\text{NH}_2\text{NO}_2\) is 0.848 M, calculate the concentration of \(\text{NH}_2\text{NO}_2\) after 28,016 seconds. Solution: \[ \_\_\_\_\_ \text{M} \] After 28,016 seconds have passed.
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