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Question

Let’s assume I want to double the rate of a reaction. The constraint is that I can only increase the temperature by 10 K. Calculate the minimum activation energy required if the temperature is 300K.


A

54 kJmol1

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B

64 kJmol1

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C

94 kJmol1

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D

84 kJmol1

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Solution

The correct option is A

54 kJmol1


Now you must be thinking that the rate constant is not given.
How do we proceed?

Let’s take some assumptions.

When T1=300 K,k1=k
When T2=300+10=310 K,k2=2k

Substituting these values in the equation

logk2k1=Ea2.303R(T2T1T1T2)

We get, log 2kk=Ea2.303×8.314×103(310300300×310)log2=Ea×1032.303×8.314×(10300×310)Ea=53.6kJmol1


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