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    krsam23 Posts: 2, Reputation: 1
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    Feb 16, 2014, 04:50 PM
    Arrhenius Equation
    1. The reaction for the decomposition of dinitrogen monoxide gas to form oxygen radicals is:
    N2O(g) --> N2(g) + O(g). If the rate constant is 0.0368 s-1 and the frequency factor is 8.00x1011 s-1, what is the activation energy for the first-order reaction at 710 degreesC? Units: kJ/mol

    What I did: ln(0.0368)=ln(8.00E11)-(ea/8.314)(1/983...
    ln(0.0368)-ln(800E11)/983.15(8.314)=-Ea
    Ea= .0037
    But the Correct answer is: 250.98

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