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Question

The rate of a reaction triples when temperature changes from 20oC to 50oC. Calculate energy of activation for the reaction. (R=8.314 J K1mol1)

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Solution

The Arrhenius equation is,

log10k2k1=EaR×2.303[T2T1T1T2]

Given: k2k1=3; R=8.314 J K1 mol1; T1=20+273=293 K
and T2=50+273=323 K

Substituting the given values in the Arrhenius equation,
log103=Ea8.314×2.303[323293323×293]

Ea=2.303×8.314×323×293×0.47730

=28811.8 J mol1 =28.8118 kJ mol1

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