The activation energy of a non-catalysed reaction at `37^(@)C` is 200 kcal/mol and the activation energy of the same reaction when catalysed decreases to only 6.0 kcal/mol. Calculate the ratio of rate constants of the two reactions.
Text Solution
AI Generated Solution
To calculate the ratio of the rate constants of a non-catalyzed reaction and a catalyzed reaction, we can use the Arrhenius equation, which relates the rate constant (k) to the activation energy (Ea) and temperature (T). The Arrhenius equation is given by:
\[ k = A e^{-\frac{E_a}{RT}} \]
Where:
- \( k \) = rate constant
- \( A \) = Arrhenius constant (frequency factor)
- \( E_a \) = activation energy
...
Topper's Solved these Questions
Chemical Kinetics
MOTION|Exercise SOLVED EXAMPLE (OBJECTIVE)|10 Videos
Chemical Kinetics
MOTION|Exercise SOLVED EXAMPLE (SUBJECTIVE)|24 Videos
CHEMICAL EQUILIBRIUM
MOTION|Exercise Exercise - 4|20 Videos
CLASSROOM PROBLEMS
MOTION|Exercise Electrochemistry|22 Videos
Similar Questions
Explore conceptually related problems
The activation energy of the reaction, A+BtoC+D+38 kcal is 20 kcal. What would be the activation energy pof the following reaction. C+DtoA+B
Activation energy of the reaction AtoB+38KCal is 20KCal. Then activation energy of reaction BtoA bill be :-
An enzyme catalyses a reaction by activation energy of the reaction .
The activation energy for an uncatalysed reaction is less than that for a catalysed reaction. What do you conclude from the above statement ?
The rate of a catalysed reaction at 27^(@)C is e^(2) times the rate of uncatalysed reaction at 727^(@)C . If the catalyst decreased the activation energy by 6 Kcal/mol, the activation energy of uncatalysed reaction is (consider the same value of pre-exponential factors in both cases):
The activation energy of exothermic reaction ArarrB is 80 kJ "mol"^(-1) . The heat of reaction is 200 kJ "mol"^(-1) . The activation energy for the reaction Brarra ( in kJ/mol) will be :
