If a temperature increase from 12. 0 °C to 20. 0 °C doubles the rate constant for a reaction. What is the value of the activation barrier for the reaction is 60.155KJ/mol.
<h3>What is activation energy? </h3>
Activation energy is defined as the minimum amount of energy required by molecules to occur a chemical reaction. It is denoted by Ea.
Given,
T1 = 12+273 = 285K
T2 = 20 +273 = 293K
Rate constant = k2/k1 = 2:1
Using arrhenius equation which give relationship between constant of reaction and temperature is
In(k2/k1) = Ea/(R[1/T1 - 1/T2]
where, Ea is the activation energy
and R is the gas constant
T1 is the initial temperature
T2 is the final temperature
In2= Ea/R[(1/285) - (1/293)]
Ea = In2 × 8.314 ×285×293/8
Ea = 0.301 ×8.314 ×285×293/8
Ea = 60155J/mol
Ea = 60.155KJ/mol.
Thus we calculated that the activation energy for a reaction at 12°C to 20°C is 60.155KJ/mol.
learn more about activation energy:
brainly.com/question/2410158
#SPJ4
