The specific reaction rate of a reaction quadruples when temperature changes from 30°C to 50°C. Calculate the energy of activation of the reaction [Given : `R = 8.314 "JK"^(-1) "mol"^(-1)` ]

Explanation

`T_1 = 30 + 273 = 303 ` K
`T_2 = 50 + 273 =323` K
`T_2 - T_1 = 323 - 303 = 20` K
`(K_2)/(K_1) = 4`
`E_a = (2.303 RT_(1) T_(2) log"" (K_2)/(K_1) )/( (T_2 - T_1 ))`
`E_a = ((2.303)(8.314) (303)(323) log 4)/( (323 - 303))`
`E_a = (2.303 (8.314)(303)(323) log 4)/( (20) )`
`E_a = 56217.3` Joule
`E_a = 56.2` kJ/mole