The decomposition of nitramide in aqueous solution at 25 °C NH2NO2(aq)------->N2O(g) + H2O(l) is first order...
The decomposition of nitramide in aqueous solution at 25
°C
NH2NO2(aq)------->N2O(g)
+ H2O(l)
is first order in
NH2NO2.
During one experiment it was found that when the initial
concentration of NH2NO2 was
0.458 M, the concentration of
NH2NO2 dropped to
0.117 M after 21860
s had passed.
Based on this experiment, the rate constant for the reaction is
_________s-1.
Homework Answers
we have:
[NH2NO2]o = 0.458 M
[NH2NO2] = 0.117 M
t = 21860.0 s
use integrated rate law for 1st order reaction
ln[NH2NO2] = ln[NH2NO2]o - k*t
ln(0.117) = ln(0.458) - k*2.186*10^4
-2.146 = -0.7809 - k*2.186*10^4
k*2.186*10^4 = 1.365
k = 6.243*10^-5 s-1
Answer: 6.24*10^-5 s-1
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