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The rate of reaction triples when temper...

The rate of reaction triples when temperature changes form `20^(@)C` to `50^(@)C`. Calculate the energy of activation for the reaction `(R= 8.314JK^(-1)mol^(-1))`.

Text Solution

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The Arrhenius equation is ,
`"log"_(10)(k_(2))/(k_(1))=(E_(a))/(Rxx2.303)[(T_(2)-T_(1))/(R_(1)T_(2))]`
Given : `(K_(2))/(k_(1))=3, R=8.314JK^(-1)"mol"^(-1),T_(1)=20+273=293K`
and `T_(2)=50+273+323K`
Substituting the given values in the Arrahenius equation,
`"log"_(10)3=(E_(a))/(8.314xx2.303)[(323-293)/(323xx293)]`
`E_(a) =(2.303xx8.314xx323xx293xx0.477)/(30)`
`=28811.8J "mol"^(-1)=28.8118 KJ"mol"^(-1)`
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