Arrhenius Equation (Dependence of Rate Constant on Temperature)

Arrhenius Equation:

Quantitatively, the effect of temperature on the rate of reaction and hence on the rate constant (k) was proposed by Arrhenius in 1889 called Arrhenius Equation. This equation is-

k = Ae^-E_a/RT

Where A = Frequency Factor, E_a = Activation Energy, R = Gas Constant, T = Temperature

In this equation, the factor e^-E_a/RT gives the fraction of molecules having energy equal to or greater than the activation energy (E_a).

Taking log to both sides of the above equation-

2.303 log k = 2.303 log (Ae^-E_a/RT) = (2.303 log A) –(E_a/RT)
⇒ log k = log A – (E_a/2.303RT) = – (E_a/2.303R) (1/T) + log A ……….(I)

Equation (I) resembles with equation of straight line, y = mx + C.

So when log k is plotted versus 1/T, we get a straight line as shown. The intercept of this line on the y-axis is equal to log A and the slope of line is equal to – E_a/2.303R.

∴ Slope = – E_a/2.303R

So, knowing the slope of equation and gas constant ‘R’ activation energy is calculated. It is the application of the Arrhenius Equation. It can alternatively be calculated by measuring two rate constants (k₁) and (k₂) at two temperatures T₁k and T₂k.

log k₁ = log A – (E_a/2.303RT₁)
and log k₂ = log A – (E_a/2.303RT₂)

∴ log k₂ – log k₁
= [log A – (E_a/2.303RT₂)] – [log A – (E_a/2.303RT₁)]
= (E_a/2.303RT₁) – (E_a/2.303RT₂)

or log (k₂/k₁)
= E_a/2.303R (1/T₁ – 1/T₂)
= E_a/2.303R [(T₂ – T₁)/T₁T₂]

Optical Fibre	Factors Affecting the Rate of Reaction
Rainbow and its Types	Molecularity of Reaction
Huygens Principle	Rate Constant and Specific Rate Constant
Self Induction	Chemical Bonding– Tamil Board