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Calculate the activation energy of the r...

Calculate the activation energy of the reaction whose rate constant for decomposition of `N_(2)O_(5) " at " 25^(@)C and 65^(@)C " are " 3.46xx10^(-5)and 4.87xx10^(-3)"min"^(-1)` respectively.

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`log.(k_(2))/(k_(1))=(E_(a))/(2.303R)xx((T_(2)-T_(1))/(T_(1)T_(2)))`
or, `log.(4.87xx10^(-3))/(3.46xx10^(-5))=(E_(a))/(2.303xx8.314)((40)/(298xx338))`
`therefore E_(a)=103.58"kJ.mol"^(-1)=24.756"kcal.mol"^(-1)`
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