The first order reaction `2N_(2)O(g)rarr2N_(2)(g)+O_(2)(g)` has a rate constant of `1.3 xx 10^(-11)s^(-1)` at `270^(@)C` and `4.5 xx 10^(-10)s^(-1)` a

Question

The first order reaction `2N_(2)O(g)rarr2N_(2)(g)+O_(2)(g)` has a rate constant of `1.3 xx 10^(-11)s^(-1)` at `270^(@)C` and `4.5 xx 10^(-10)s^(-1)` a

The first order reaction `2N_(2)O(g)rarr2N_(2)(g)+O_(2)(g)` has a rate constant of `1.3 xx 10^(-11)s^(-1)` at `270^(@)C` and `4.5 xx 10^(-10)s^(-1)` at `350^(@)C`. What is the activation energy for this reaction ?
A. 15 kJ
B. 30 kJ
C. 68 kJ
D. 120 kJ

Monjur Alahi

5 views

2025-01-04 04:42

1 Answers

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Salim Ahmed Kawsar · Accepted Answer · 2023-02-05T15:29:48+06:00

Salim Ahmed Kawsar

`log((k_(2))/(k_(1)))=(E_(a))/(2.303R)[(1)/(T_(1))-(1)/(T_(2))]`
`log ((4.5xx10^(-10))/(1.3xx10^(-11)))=(E_(a))/(2.303xx8.314xx10^(-3))[(1)/(543)-(1)/(623)]`
`E_(a)=120 kJ`

5 views Answered 2023-02-05 15:29