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Arrhenius equation - The effect of temperature on reaction rate
Generally, the rate of a reaction increase with increasing temperature. However, there are very few exceptions. The magnitude of this increase in rate is different for different reactions. As a rough rule, for many reactions near room temperature, reaction rate tends to double when the temperature is increased by 10ºC .
A large number of reactions are known which do not take place at room temperature but occur readily at higher temperatures. Example: Reaction between H2 and O2 to form H2O takes place only when an electric spark is passed.
Arrhenius suggested that the rates of most reactions vary with temperature in such a way that the rate constant is directly proportional to e-(E0/RT) and he proposed a relation between the rate constant and temperature.
Where A the frequency factor,
R the gas constant,
Ea the activation energy of the reaction and,
T the absolute temperature (in K)
The frequency factor (A) is related to the frequency of collisions (number of collisions per second) between the reactant molecules. The factor A does not vary significantly with temperature and hence it may be taken as a constant.
Ea is the activation energy of the reaction, which Arrhenius considered as the minimum energy that a molecule must have to posses to react.
Taking logarithm on both side of the equation (1)
The above equation is of the form of a straight line y = mx + c.
A plot of ln k Vs 1/T gives a straight line with a negative slope – Ea/R. If the rate constant for a reaction at two different temperatures is known, we can calculate the activation energy as follows.
At temperature T = T1 ; the rate constant k = k1
At temperature T = T2 ; the rate constant k = k2
This equation can be used to calculate from rate constants k1 and k2 at temperatures T1 and T2 .
The rate constant of a reaction at 400 and 200K are 0.04 and 0.02 s-1 respectively. Calculate the value of activation energy.
According to Arrhenius equation
Ea = 2305 J mol−1
Rate constant k of a reaction varies with temperature T according to the following Arrhenius equation
Where Ea is the activation energy. When a graph is plotted for log k Vs 1/T a straight line with a slope of - 4000K is obtained. Calculate the activation energy
Ea = − 2.303 R m
Ea = − 2.303 x 8.314 J K−1 mol−1 x (− 4000K )
Ea = 76,589J mol−1
Ea = 76.589 kJ mol−1
For a first order reaction the rate
constant at 500K is 8 X 10−4 s−1 . Calculate the
frequency factor, if the energy of activation for the reaction is 190 kJ mol-1
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