Rate constant k of a reaction varies with temperature T according to the equation
1
log log
2.303
Ea K A
R T
. When a graph of log k is plotted vs
1
T
, a straight line
with slope -4250 is obtained. Calculate the energy of activation. (Given R =
8.314J/Kmol
Answers
Answer:
with slope -4250 is obtained. Calculate the energy of activation. (Given R =
8.314J/Kmol
Explanation:
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.