The half life of first order decomposition of nitramide is 2.0 hour at `15^@C`.
`NH_2NO_2(aq) to N_2O(g) + H_2O(l)` If 6.2 gm of `NH_2NO_2` is allowed to decompose, find :
time taken for nitramide to decompose 99%

Explanation

To solve the problem of the time taken for nitramide (NH₂NO₂) to decompose 99%, we can follow these steps:

### Step 1: Understand the Reaction and Given Data
We know that the decomposition of nitramide is a first-order reaction, and the half-life (t₁/₂) is given as 2.0 hours at 15°C. The reaction is:
\[ \text{NH}_2\text{NO}_2(aq) \rightarrow \text{N}_2\text{O}(g) + \text{H}_2\text{O}(l) \]

### Step 2: Calculate the Rate Constant (k)
For a first-order reaction, the relationship between the half-life and the rate constant (k) is given by:
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