Advertisements
Advertisements
प्रश्न
Show that the time required for 99% completion is double of the time required for the completion of 90% reaction.
For a first-order reaction, derive the relationship t99% = 2t90%.
Advertisements
उत्तर
For Ist order reaction k = `2.303/"t" log (["A"_0])/(["A"_"t"])`
For 99% completion: If [A0] = 100
[At] = 100 − 99
= 1
∴ t99% = `2.303/"k" log 100/1`
t99% = `2.303/"k" xx 2` .........(1)
∵ log 100 = 2
For 90% completion: If [A0] = 100
[At] = 100 − 90
= 10
t90% = `2.303/"k" log 100/10`
t90% = `2.303/"k"` ...........(2)
∵ log 10 = 1
From (1) and (2),
t99% = 2t90%
APPEARS IN
संबंधित प्रश्न
The integrated rate equation for first order reaction is A → products
For a first order reaction, show that time required for 99% completion is twice the time required for the completion of 90% of reaction.
A first order reaction takes 30 minutes for 50% completion. Calculate the time required for 90% completion of this reaction.
(log 2 = 0.3010)
During nuclear explosion, one of the products is 90Sr with half-life of 28.1 years. If 1μg of 90Sr was absorbed in the bones of a newly born baby instead of calcium, how much of it will remain after 10 years and 60 years if it is not lost metabolically?
Show that for a first order reaction half life is independent of initial concentration.
The rate constant for a first order reaction is 1.54 × 10−3 s−1. Calculate its half life time.
The half life of the homogeneous gaseous reaction \[\ce{SO2Cl2 -> SO2 + Cl2}\] which obeys first order kinetics is 8.0 minutes. How long will it take for the concentration of SO2Cl2 to be reduced to 1% of the initial value?
The half-life of cobalt 60 is 5.26 years. The percentage activity remaining after 4 years is ______%.
The rate of a first order reaction is 0.04 mol litre-1 s-1 at 10 minutes and 0.03 mol litre-1 sec-1 at 20 minutes after initiation. The half-life of the reaction is ______ min.
The half-lives of a first-order reaction are 1.19s at 313 K and 15.45s at 293 K. Calculate the energy of activation.
