The rate constant for the order reaction increases from `4 xx 10^(-2)` to `24 xx 10^(-2)` when the temperature changes from 300K to 350 K. Calculate e

Question

The rate constant for the order reaction increases from `4 xx 10^(-2)` to `24 xx 10^(-2)` when the temperature changes from 300K to 350 K. Calculate e

The rate constant for the order reaction increases from `4 xx 10^(-2)` to `24 xx 10^(-2)` when the temperature changes from 300K to 350 K. Calculate energy of activation for this reaction.

Monjur Alahi

4 views

2025-01-04 04:42

1 Answers

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

According to the avialable data,
`k_(1)=4 xx 10^(-2), k_(2)=24 xx 10^(-2), T_(1)=300K, T_(2)=350K` ,
According to Arrhenius equation:
`log k_(2)/k_(1) = E_(a)/(2.303R) [1/T_(1)-1/T_(2)]`
`log (24 xx 10^(-2))/(4 xx 10^(-2)) = (E_(a))/(2.303 xx8.314 J mol^(-1))[1/300K-1/350K]`
`log6 = =(E_(a))/(2.303 xx 8.314 J mol^(-1))[(50)/(300 xx 350)]`
`K_(a) = (0.7782 xx 2.303 xx 8.314 J mol^(-1) xx 300 xx 350)/(50)`
`=31290 J mol^(-1)=31.290 kJ mol^(-1)`