Question

A reaction has activation energy of 85kjper mol. What is the effect on the rate of raising the temperature from 20degree to 30 degree​

Answer 1

Answer: The rate increases 3 times on raising the temperature from 20degree to 30 degree​

Step-by-step explanation:

According to Arrhenius equation with change in temperature, the formula is as follows.

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

where
`k_2` = rate constant at temp
`T_2`

`k_1` = rate constant at temp
`T_1`

`E_a`= activation energy

R= gas constant

`T_1`= temperature =
`20^0C=(20+273)K=293K`

`T_2`= temperature =
`30^0C=(30+273)K=303K`

`ln (k_(2))/(k_(1)) = (-85* 1000J/mol)/(8.314J/Kmol)[(1)/(303) - (1)/(293)]`

`ln (k_(2))/(k_(1))=1.15`

`(k_(2))/(k_(1))=3`

Thus rate increases 3 times on raising the temperature from 20degree to 30 degree​