Question

When the temperature of a reaction is raised from 278 K to 300 K, the reaction rate increases by a factor of 17. Determine the activation energy, Ea, of the reaction. R = 8.314 J/mol.K

Answer 1

Answer: The activation energy, Ea, of the reaction is 89195 Joules

Step-by-step explanation:

The effect of temperature on rate constant is given by Arrhenius equation:

`ln (k_(2))/(k_(1)) = (-E_(a))/(R)[(1)/(T_(2)) - (1)/(T_(1))]`

where

`k_2` = rate constant at temperature
`T_2`

`k_1` = rate constant at temperature
`T_1`

`E_a`= activation energy

R= gas constant

`T` = temperature

`ln (17k_1)/(k_(1)) = (-E_(a))/(8.314)[(1)/(300) - (1)/(278)]`

`2.83=(-E_(a))/(8.314)[(1)/(300) - (1)/(278)]`

`E_a=89195J`

The activation energy, Ea, of the reaction is 89195 Joules