2. Introduction
It is a formula for the temperature
dependence of reaction rates.
Proposed by Mr. Svante Arrhenius in 1889
based on the Dutch chemist, Mr. Jacobus
HenricusVan’t Hoff.
3. It gives the dependence of rate constant(k)
of a chemical reaction on the absolute
temperature.
5. Purposes of Arrhenius equation:
Verify the effect ofTemperature, catalyst, Gas
constant.
Temperature,T
To fit, this should be in Kelvin.
The gas constant, R
Which comes from the PV=nRT
6. Activation energy, E
Minimum energy for reaction to occur.
The e=2.7182
The frequency factor, A:
A term which includes factors like frequency
of collisions and their orientations.
7. Uses of Arrhenius equation:
Used extensively to describe the effect of
temperature;Thermal death.
To determine how the reac. rates and
diffusion changes with temperature.
8. Effect of Temeperature:
On raising the temperature atleast for 10
degree centigrade, the rate constant gets
doubled.
Therefore, we can say that, the rate constant
is directly proportional to the temperature.
9. Effect of catalyst:
A catalyst provides route for the reaction
with a lower activation energy.
On adding the catalyst..
10. Frequency factor
The frequency factor A is considered to be a
constant and has very less effect on the
varience of rate constant.
11. Conclusion:
Therefore, with the help of the
Arrhenius equation we came to
know that, the rate constant is
also dependent upon the
temperature, gas constant,
catalyst etc..
