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Half life period of a reaction:
The half life of a reaction is defined as the time required for the reactant concentration to reach one half its initial value. For a first order reaction, the half life is a constant i.e., it does not depend on the initial concentration.
The rate constant for a first order reaction is given by
Let us calculate the half life period for a zero order reaction.
Hence, in contrast to the half life of a first order reaction, the half life of a zero order reaction is directly proportional to the initial concentration of the reactant.
A first order reaction takes 8 hours for 90% completion. Calculate the time required for 80% completion. (log 5 = 0.6989 ; log10 = 1)
For a first order reaction,
Let [A0 ] = 100M
t = t90% ; [A]=10M (given that t90 % =8hours)
t = t80% ; [A]=20M
Find the value of k using the given data
Substitute the value of k in equation (2)
t80% = 8hours x 0.6989
t80% = 5.59hours
(ii) The half life of a first order reaction x → products is 6.932 x 104s at 500K . What percentage of x would be decomposed on heating at 500K for 100 min. (e0.06 = 1.06)
Given t1/2 = 0.6932 x 104 s
To solve :2 when t=100 min,
[ [A0 ] −[A] / [A0] ] x 100 = ?
We know that
For a first order reaction, t1/2 = 0.6932 / k
k = 10−5 s−1
Show that in case of first order reaction, the time required for 99.9% completion is nearly ten times the time required for half completion of the reaction.
1. In a first order reaction A → products 60% of the given sample of A decomposes in 40 min. what is the half life of the reaction?
2. The rate constant for a first order reaction is 2.3 X 10 −4 s−1 If the initial concentration of the reactant is 0.01M . What concentration will remain after 1 hour?
3. Hydrolysis of an ester in an aqueous solution was studied by titrating the liberated carboxylic acid against sodium hydroxide solution. The concentrations of the ester at different time intervals are given below.
Show that, the reaction follows first order kinetics.
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