The rate constant for first order reaction becomes six times when the temperature is raised from 50 K to 400 K. Calculate the activation energy for the reaction. (R= 8.314 J/K/mol)

Explanation

`"log" (6k)/(k) = (E_a)/(19.17)[(400 - 350)/(140000)]`
`0.9542 = (E_a)/(19.17) [15/140000]`
`E_a = (0.7788 xx 19.17 xx 14000)/(5)`
` E_a = 41.758 kJ mol^(-1)`