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16 October, 00:50

HI (g) + CH3I (g) - > CH4 (g) + I2 (g) the rate constant is 0.28 L/Mol*s at 300*C and 0.0039 L/Mol*s at 227*C. a) What is the Activation energy of this reaction. b) What is k at 400*C

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  1. 16 October, 04:34
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    (a) The activation energy (Ea) is 3284.6 L. atm/mol

    (b) At 400°C, k is 0.6579 L/Mol*s

    Explanation:

    (a) The activation energy for the reaction is determined using Arrhenius equation

    In (k2/k1) = - Ea/2.303R [1/T2 - 1/T1]

    k2 = 0.28 L/mol*s, k1 = 0.0039 L/mol*s, R = 0.082057 L. atm/molK, T2 = 300°C = 300+273K = 573K, T1 = 227°C = 227+273K = 500K

    In (0.28/0.0039) = - Ea/2.303*0.082057 [1/573 - 1/500]

    4.27 = - Ea (-0.0013)

    4.27 = 0.0013Ea

    Ea = 4.27/0.0013 = 3284.6 L. atm/mol

    (b) The value of k at 400°C is determined by interpolation

    T (°C). Rate constant (L/mol*s)

    227. 0.0039

    300 0.28

    400 k

    400-227/300-227 = k-0.0039/0.28-0.0039

    2.37 = k-0.0039/0.2761

    k-0.0039 = 2.37*0.2761

    k-0.0039 = 0.654

    k = 0.654+0.0039 = 0.6579L/mol*s
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