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The value of rate constant for the decom...

The value of rate constant for the decomposition of nitrogen pentoxide `(N_(2) O_(s) to N_(2) O_(4) + (1)/(2) O_(2) )` is `3.46 xx 10^(-5)` at `25^(@) C and 4.87 xx 10^(-3)` at `65^(@) C`. Calculate the energy of activation for the reaction. (`R = 8.314JK^-1mol^-1`)

Text Solution

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Here, `k_1 = 3.46 xx 10^(-5) T_1 = 273 + 25 = 298K`
`k_2 = 4.87 xx 10^(-3) T_2 = 273 + 65 = 338K`
`therefore " "log"" (k_2)/(k_1) = (E_a)/( 2.303R) [(T_2- T_1)/(T_2 T_1) ]`
Putting the values in the above equation,
We get `E_a = 24,800 " cal" = 24.8 " kcal"`.
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