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Question

In the Arrhenius equation for a certain reaction, the value of A and E (energy of activation) are 4×1013sec1 and 98.6 kJ mol1 respectively. If the reaction is of the first order, the temperature at which its half-life period will be 10 minutes in K will be x, then find the value of x/6 to the nearest integer.

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Solution

Given: A=4×1013sec1

Ea=98.6×103Jmol1,t1/2=10×60sec

K=AeEa/RT

K=4×1013×e[(98.6×103)/(8.314×T)]

For 1st order reaction K=(0.693/t1/2)=(0.693/600)sec1

(0.693/600)=4×1013×e[(98.6×103)/(8.314×T)]
Take log both side-

log(0.693/600)=log(4×1013)(98.6×103)(8.314×2.303T)

T=415.3K
x/6=70

Answer is 70.

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