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26 June, 06:42

For the reaction given below, the frequency factor A is 8.7 1012 s-1 and the activation energy is 63 kJ/mol. NO (g) + O3 (g) → NO2 (g) + O2 (g) What is the rate constant for the reaction at 70°C?

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  1. 26 June, 07:09
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    K (70°C) = 2213.376 s-1

    Explanation:

    balanced reaction:

    NO (g) + O3 (g) → NO2 (g) + O2 (g)

    ∴ Ea = 63 KJ/mol

    ∴ A = 8.7 E12 s-1

    ∴ T = 70°C ≅ 343 K

    Arrhenius eq:

    K (T) = Ae∧ ( - Ea/RT)

    ∴ R = 8.314 E-3 KJ/K. mol

    ⇒ K (70°C) = (8.7 E12 s-1) e∧[ - (63) / (8.314 E-3) (343) ]

    ⇒ K (70°C) = (8.7 E12 s-1) * (2.5444 E-10)

    ⇒ K (70°C) = 2213.376 s-1
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