Home
Class 12
CHEMISTRY
How much faster would a reaction proceed...

How much faster would a reaction proceed at `25^(@)C` than at `0^(@)C` if the activation energy is `65 kJ`?

A

`2 "times"`

B

`16 "times"`

C

`11 "times"`

D

`6 "times"`

Text Solution

Verified by Experts

The correct Answer is:
c
`2.303"log"K_(2)/K_(1)=E_(a)/R[(T_(2)-T_(1))/(T_(1)T_(2))]`
`:. 2.303"log"K_(2)/K_(1)=(65xx10^(3))/(8.314)[(25)/(298xx273)]`
`:. K_(2)/K_(1)=11.05`
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL KINETICS

    P BAHADUR|Exercise Exercise 1|2 Videos

  • CHEMICAL KINETICS

    P BAHADUR|Exercise Exercise 3A|2 Videos

  • DILUTE SOLUTION AND COLLIGATIVE PROPERTIES

    P BAHADUR|Exercise Exercise 9 Advanced Numerical|12 Videos

Similar Questions

Explore conceptually related problems

The rate of reaction ((dx)/(dt)) varies with nature, physical state and concentration of reactants, temperature, exposure to light and catalyst, whereas rate constant (K) varies with temperature and catalyst only. The rate constant K is given as K=Ae^(-E_(a)//RT) where A is Arrhenius parameter or pre-exponential factor and E_(a) is energy of activation. The minimum energy required for a reaction is called threshold energy and the additional energy required by reactant molecules to attain threshold energy level is called energy of activation. How much faster would a reaction proceed at 25^(@)C than at 0^(@)C if the activation energy is 2 cal?

The rate of a reaction at 75^(@) C is 30.0 times that at 25^(@) C . What is its activation energy?

The rate constant is doubled when temperature increases from 27^(@)C to 37^(@)C . Activation energy in kJ is

A reaction proceeds five times more at 60^(@)C as it does at 30^(@)C . Estimate energy of activation.

For a certain gaseous reaction rise of temperature from 25^(@)C to 35^(@)C doubles the rate of reaction. What is the value of activation energy :-

Assertion (A) : If the activation energy of a reaction is zero, temperature will have no effect on the rate constant. Reason (R ): Lower the activation energy, faster is the reaction.