Home
Class 12
CHEMISTRY
In general it is observed that the rate ...

In general it is observed that the rate of a chemical reaction becomes double for every `10^@` rise in temperature. If this generalisation holds for a reaction in the temperature range 2908 K to 398 K, what would be the value of activation energy for the reaction.
(R=8.314 J `K^(-1)mol^(-1)`)

Text Solution

Verified by Experts

`"log" (k_2)/(k_1) = (E_a)/(2.303) [1/(T) - 1/(T_2)] " " [A.E.]`
`(k_2)/(k_1) =2 `(given in question)
`log 2 = (E_a)/(2.303 xx 8.314)[1/298 - 1/308]`
`E_a = (0.3010 xx 2.303 xx 8.314 xx 298 xx 308)/(10)`
`E_a = 52898 J mol `
`E_a = 52.898 KJ mol^(-1)`
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • CHEMICAL KINETICS

    ACCURATE PUBLICATION|Exercise TOPIC : CHEMICAL KINETIC|69 Videos
  • CHEMICAL KINETICS

    ACCURATE PUBLICATION|Exercise NUMERICAL OF HALF LIFE TIME PERIOD |6 Videos
  • BOARD PAPER MARCH - 2020

    ACCURATE PUBLICATION|Exercise SECTION - D|18 Videos
  • COORDINATION COMPOUNDS

    ACCURATE PUBLICATION|Exercise 2 MARKS QUESTIONS|23 Videos

Similar Questions

Explore conceptually related problems

In General it is observed that the rate of a chemical reaction becomes double for every 10^@ rise in temperature. If this general is action holds for a reaction in the temperature range 298 K to 308 K. What would be the value of activation energy for the reaction.

The rate of a chemical reaction becomes double for every 10^@C rise in temperature. If this generalisation holds for a reaction in the temperature range 290 K to 300 K, what would be the approximate value of E_a for the reaction ?

Knowledge Check

  • The rate of chemical reaction becomes double for every 10^@ rise in temperature because of

    A
    increase in activation energy
    B
    decrease in activation energy
    C
    increase in number of molecular collisions
    D
    increase in number of activated molecules
  • The rate of chemical reaction double for every 10^@С rise of temperature if the temperature is raised by 50^@C , the rate of the reaction increases by

    A
    10 times
    B
    24 times
    C
    32 times
    D
    64 times
  • Similar Questions

    Explore conceptually related problems

    The rate constant of a reaction increases four times when the temperature changes from 300 K to 320 K, Calculate the activation energy for the reaction. (R = 8.314 Jmol ^(-1) K ^(-1))

    The rate constant for first order reaction becomes six times when the temperature raised from 350 to 400 K. Calculate the activation energy for the reaction. (R = 8.314 J/ K/mol)

    The rate of reactions become double by rise of 10^@ temperature. Explain

    The rate constant for first order reaction becomes six times when the temperature is raised from 50 K to 400 K. Calculate the activation energy for the reaction. (R= 8.314 J/K/mol)

    The rate constant for a first order reaction becomes six times when the temperature is raised from 350 K to 400 K. Calculate activation energy for the reaction.

    The rate of a reaction doubles when its temperature changes from 300 K to 310 K Activation energy of such a reaction will be (R = 8.314 JK^-1 mol^-1 and log 2 = 0.301)