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Question

Calculate the activation energy for a reaction of which rate constants becomes 4 times when temperature changes from 300C to 500C [R= 8.314 Jmol1K1]

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Solution

lnkk=EaR×[TTTT]
T=30 oC=30+273 K=303 K
T=50 oC=50+273 K=323 K
lnkk=EaR×[TTTT]
ln4kk=Ea8.314 J/mol/K×[323303303×323]
1.386=2.46×105×Ea
Ea=56400 J/mol
Ea=56.4 kJ/mol
because 1 kJ=1000 J
Note: Since rate constant becomes 4 times, k=4k

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