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A reaction has rate constants 1.73 xx...

A reaction has rate constants `1.73 xx 10^(-3) min^(-1) ` and `4.86 xx 10^(-3) min^(-1) ` at 300 K and 300 K respectively. Calculate
The energy of activation of the reaction
`(R= 8.314 JK^(-1) mol^(-1))`

Text Solution

Verified by Experts

Activation energy `=E_(a) = 28. 35 kJ`
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Knowledge Check

  • The rate constant for a reaction is 2xx10^(-2) s^(-1) at 300 K and 8xx10^(-2) s ^(-1) at 340 K The energy of activation of the reaction is

    A
    `14.695` kJ `"mol"^(-1)`
    B
    `29.39` kJ `"mol"^(-1)`
    C
    `44 kJ "mol"^(-1)`
    D
    `22 kJ "mol"^(-1)`

  • The rate coefficient (k) for a particular reactions is 1.3 xx 10^(-4)M^(-1)s^(-1) at 100^(@)C , and 1.3 xx 10^(-3)M^(-1)s^(-1) at 150^(@)C . What is the energy of activation ( E_(a) ) (in kJ) for this reaction? (R=molar gas constant = 8.314 JK^(-1) mol^(-1) )

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    B
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    99
    D
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  • A plot of "Ink "v//s " 1/T" for a reaction gives the slope -1xx10^(4)k. The energy of activation for the reaction is (Given,R=8.314k^(-1)" mol"^(-1))

    A
    `8314kJ" mol"^(-1)`
    B
    `1.202kJ" mol"^(-1)`
    C
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    D
    `83.14kJ" mol"^(-1)`

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