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Question

The rate constant of a reaction at 300 K is 5.0×104minute1. The temperature was increased by 20 K and the value of rate constant K increased three times. Calculate the energy of activation of the reaction?
What will be the value of rate constant at 37C? [R=1.987 calori.Kelvin1.mol1].

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Solution

Using Arrheneius equation we get
lnk=EaRTln(k1k2)=EaR(1T21T1)
on substitution we get:
ln(5×1043×5×104)=Ea1.987(13201300)
Ea=10478.12 cal/mol
Rate constant at 37C T=310 K
lnk=10478.121.987×310=17.01k=4.09×108

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