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13 April, 03:52

Use the value of the activation energy (Ea=1.50*102kJ/mol) and the given rate constant of the reaction at either of the two temperatures to predict the rate constant at 551 K.

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  1. 13 April, 07:25
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    Answer: The rate constant

    K = 0.967m-1s-1

    Explanation: To calculate the rate constant, we will use the Arrhenius equation.

    lnK = ( - Ea/R) (1/T) + lnZ ... (1)

    K is the rate constant

    Ea is the activation energy

    R is the gas constant

    T is the temperature in Kelvin

    Z is the constant related to the geometry needed, but in this question Z is equal to zero.

    Therefore fro data given, we have

    Ea = 1.50 * 102kj/mol = 153kj/mol

    R = 8.314j/mol-k

    T = 551k

    Z = 0

    Therefore using the equation

    lnK = - 153: (8.314 * 551) = - 153 * 4581.014

    lnK = - 0.033398719

    Taking the ln inverse of K

    K = e^ (-0.033398819) = 0.96715286

    K = 0.967m-1s-1

    This is the rate constant
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