Jade asked in Science & MathematicsChemistry · 2 months ago

A certain reaction has an activation energy of 60.0 kJ/mol and a frequency factor ?

A certain reaction has an activation energy of 60.0 kJ/mol and a frequency factor of A1 = 7.80×1012 M−1s−1 . What is the rate constant, k, of this reaction at 23.0 ∘C ?

4 Answers

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  • 2 months ago

    Eₐ = 60 kJ/mol = 60000 J mol⁻¹

    R = 8.314 J mol⁻¹ K⁻¹

    T = (273.2 + 23.0) K = 296.2 K

    A = 7.80 × 10¹² M⁻¹ s⁻¹

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  • Bobby
    Lv 7
    2 months ago

    k = A e^-Ea/RT 

    k= 7.80×10^12 M−1s−1 . e^ -60kj/mol /0.0083144kj/mol.K * 296K

  • Dr W
    Lv 7
    2 months ago

    use the arrhenius equation

    .. k = Ao exp(-Ea / RT)

  • 2 months ago

    According to Arrhenius Equation:

    K = Ae^(-Ea/RT);

    K = (7.80*10^12 M−1s−1)e^((-60000 J/mol)/(8.314 J/K·mol)(296.15 K))

    K = (7.8*10^12)e^((-60000 )/((8.314)*(296.15))

    K = 6.80 x 10^(12)

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