The rate of a particular reaction triples when the temprature is increased from 25C to 35C. Calculate the activation energy for this reaction.
Also i just need to clearify the concept of Arrhenius Equation. What happened to Rate Constant(k) and the rate of reaction if:
a. there is a decrease in temperature
b. an increase in activation energy of the forward and reverse reactions. and the last is if there is an increase in both activation energy and temperature. I want to know the effect of each on Rate constant and rate of reaction
Please find the answers to your questions in the attached file.
The activation energy is given by the following formula
ln k1 / k2 = Ea / R [ 1/T2 - 1/T1 ]
Now , as per the question , k2 / k1 = 3
Ea is the activation energy
T2 = 35 C = 273 + 35 = 308 K
T1 = 25 C = 273 + 25 = 298 ...
The solution attaches a .doc file including calculations for finding the activation energy with temperature increase as well as an explanation of the Arrhenius Equation.