The half-life for the first order decomposition of nitramide is 2.1 hours at 15oC.
NH2NO2 (s) → N2O(g) + H2O(l)
If 6.2 g of NH2NO2 is allowed to decompose, calculate the time taken for 99% decomposition of NH2NO2.
Answer & explanation
Correct answer: option 2
k = \(\frac{2.303}{t}\)log\(\frac{A_o}{A}\)
Initial moles of nitramide = \(\frac{6.2}{62}\) = 0.1
∴ t = \(\frac{2.303 × 2.1}{0.693}\)log\(\frac{0.1}{0.001}\) = 13.95 hour