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Define activation energy. What is Arrhen...

Define activation energy. What is Arrhenius equation?

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The energy required to form the intermediate, called activated complex is known as activation energy `(E_a)`. The temperature dependence of rate of chemical reaction is expressed by Arrhenius equation,
`k=Ae^(-E_(a) // RT)`
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Knowledge Check

  • Arrhenius equation is :

    A
    k = -Ae^(-E_(a)/RT)
    B
    k = Ae^(-E_(a)/RT)
    C
    k = e^(-E_(a)/RT)
    D
    k = Ae^(E_(a)/RT)

  • Activation energy of a reaction is:

    A
    The energy released during the reaction
    B
    The energy evolved when activated complex is formed
    C
    Minimum amount of energy needed to overcome the potential barrier of reaction
    D
    The energy needed to form one mole of the product

  • Activation energy of a reaction is:

    A
    The energy released during the reaction
    B
    The energy evolved when activated complex is formed
    C
    Minimum amount of energy needed to overcome the potential barrier of reaction
    D
    The energy needed to form one mole of the product

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    The rate constant, the activation energy and the Arrhenius parameter of a chemical reaction at 25^@C are 3.0xx10^-4S^-1, 104.4 kj mol^-1 and 6.0xx10^14 s^-1 respectively. The value of the rate constant as T to oo is:

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