The decomposition of P2O5 is given by: rate = k[P2O5]. If the half-life for this reaction is 1400 s, about how long does it take for the P2O5 concentration to drop from 3.0 M to 0.3 M?
(1) 200 s
(2) 3000 s
(3) 4000s
(4) 4210 s
(5) 4650 s
The answer is (5) 4650s but I'm not sure how they got that. Please help, thanks!
By seeing the rate law, we can say that it is 1st order reaction
Given:
Half life = 1400 s
use relation between rate constant and half life of 1st order reaction
k = (ln 2) / k
= 0.693/(half life)
= 0.693/(1400)
= 4.95*10^-4 s-1
we have:
[P2O5]o = 3.0 M
[P2O5] = 0.3 M
k = 4.95*10^-4 s-1
use integrated rate law for 1st order reaction
ln[P2O5] = ln[P2O5]o - k*t
ln(0.3) = ln(3) - 4.95*10^-4*t
-1.204 = 1.0986 - 4.95*10^-4*t
4.95*10^-4*t = 2.3026
t = 4650 s
Answer: option 5
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