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What is the activation energy for a reac...

What is the activation energy for a reaction if its rate doubles when the temperature is raised from 200 K to 400 K ? `(R = 8.314 JK^(-1)mol^(-1))`

A

`234.65"kJ mol"^(-1)K^(-1)`

B

`434.65 "kJ mol"^(-1)K^(-1)`

C

`434.65"J mol"^(-1)K^(-1)`

D

`334.65"J mol"^(-1)K^(-1)`

Text Solution

Verified by Experts

The correct Answer is:
C
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If the rate of a reaction gets doubled as the temperature is increased from 27^(@)C to 37^(@)C . Find the activation energy of reaction ?

DeltaH and DeltaS for the reaction Ag_(2)O_((s))rarr2Ag_((s))+1/2O_(2_((g))) " are "30.56 kJ mol^(-1) and 66.0 Jk^(-1) mol^(-1) respectively. Calculate the temperature at which the free energy for this reaction will be zero. What will be the direction of reaction at this temperature and at temperature below this and why ? Given: DeltaH=30.56kJ mol^(-1)=30560 J mol^(-1) DeltaS=66.0JK^(-1)mol^(-1) DeltaG=0

Knowledge Check

  • What is the activation energy for a reaction if it rate doubles when the temperature is raised from 200 K to 400 K? (R = 8.314 JK^(-1) mol^(-1) )

    A
    `234.65 kJ mol^(-1) K^(-1)`
    B
    `434.65 kJ mol^(-1) K^(-1)`
    C
    `434.65 J mol^(-1) K^(-1)`
    D
    `334.65 J mol^(-1) K^(-1)`

  • What is the activation energy for a reaction if its rate doubles when the temperature is raised from 200K to 400 K ? ( "R"=8.314"JK"^(-1)"mol"^(-1) )

    A
    `234.65 "kJ mol"^(-1)"K"^(-1)`
    B
    `434.65"kJ mol"^(-1)"K"^(-1)`
    C
    `434.65 "J mol"^(-1)"K"^(-1)`
    D
    `334.65 "J mol"^(-1)"K"^(-1)`

  • What is the activation energy for a reaction if its rate doubles when the temperature is raised from 200 K to 400 K ? (R= 8.314"kJ"mol^(-1)K^(-1))

    A
    `234.65"kJ mol"^(-1)K^(-1)`
    B
    `434.65"kJ mol"^(-1)K^(-1)`
    C
    `434.65"J mol"^(-1)K^(-1)`
    D
    `334.65"kJ mol"^(-1)K^(-1)`

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