In: Chemistry
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The following hydrolysis reaction of an active drug follows standard first order kinetics.
Reaction: Drug + H_2O \rightarrow Hydrolyzed Drug
The initial concentration is 0.010 M and the rate constant for the reaction is 1.5E-3, the concentration 6.0E2 minutes after the patient has taken the drug is ________ (do not include units in your answer)
Based on the information above, the half life of this drug would be _________ (do not include units in your answer)
First order reaction given.
Drug + H_2O \rightarrow Hydrolyzed Drug
rate law for a first order reaction ,
rate , r = K[drug]
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To derive first order integral rate equation
r = K[drug]
let reactant , A= drug
Integration on both sides,
Homogenisation ,
Giving limits for both A and t
Ao = initial concetration of drug
A = cocnetration of drug at time t s.
k = rate constant
But we have ,
and therefore
lnx = 2.303
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Ao = initial concetration of drug
= 0.010 M
A = cocnetration of drug at time t s.
= ?
k = rate constant
= 1.5e-3
= 0.0015/m
time , t= 6.0e2
= 6.0 * 100 minutes
= 600 minutes
0.3908 = log0.010- logA
logA = -2-0.3908
= -2.3908
A = 10^-2.3908
= 0.00406 M
Answer
Concetration of drug after given time = 0.004 |
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Half life of drug
substitute,
= 462 minutes
Answer
half life of drug =
462 |