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The rate constant k of a reaction incre...

The rate constant k of a reaction increases three fold when temperature changes from `127^(@)` C to `45^(@)` C calculate the energy of activation for this reaction

Text Solution

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According to Arrhenius equation,
`log""(k_(2))/(k_(1)) = (E_(a))/(2.303 R)[(1)/(T_(1)) - (1)/(T_(2))]` or `log""(k_(2))/(k_(1)) = (E_(a))/(2.303 R)[(T_(2)-T_(1))/(T_(1)T_(2))]`
`log""(3)/(2) = (E_(a))/(2.303 xx 8.314 J mol^(-1) K^(-1)) xx (18)/(300 xx 318)`
`0.4771 = (E_(a))/(2.303 xx 8.314 J mol^(-1)) xx (18)/(300 xx 318)`
`E_(a) = (0.4771 xx 2.303 xx 8.314 xx 300 xx 318)`
`E_(a) = (0.4771 xx 2.303 xx 8.314 xx 300 xx 318)/(18) mol^(-1)`
`=48416.03 J mol^(-1)`
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