At a certain temperature this reaction follows second-order kinetics with a rate constant of 2.2 M^-1s^-1.
2NH3 à N2 + 3H2
Supposes a vessel contain NH3 at a concentration of 0.920 M. calculate how long it takes for the concentration of NH3 to decrease by 92%. You may assume no other reaction is important.
2 significant digits.
Please show me steps.. thank you
initial = 0.920 M = Ao
remaining = 0.920 – 0.920 x 92 / 100
= 0.0736 M
k = 2.2 M-1 s-1
for second order reaction formula :
t = 1/ k [1 / At – 1 / Ao]
t = 1/ 2.2 [1/0.0736 – 1/ 0.920]
t = 5.68 sec
time = 5.7 sec
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