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chemistry

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Values of the rate constant for the decomposition of N2O5 at four different temperatures are as follows:

T(K) k(s^-1)
658....2.14*10^5
673....3.23*10^5
688....4.81*10^5
703....7.03*10^5

The activation energy is 1.02*10^2 kJ/mol. Calculate the value of the rate constant at 300 K

  • chemistry -

    Can't you use the Arrhenius equation?
    Use two T values with corresponding k values. One T will be 300 and k at that T will be the unknown.

  • chemistry -

    I keep trying that and it is saying that I have the wrong answer. here is my work:

    slope: -1.19*10^4 y-intercept= 30.439

    Ea: -(-1.19*10^4 K) *(8.314J/moK)= 9.89*10^4 J/mol

    A= e^30.439= 1.65*10^13

    (1.65*10^13) e^-(9.89*10^4J/mol/8.314*300 K)= 9.98*10^-5

    I keep getting different answers, and each time they are saying it is wrong. Can you tell me where I am going wrong? And am I supposed to convert the Ea into joules/mole?

  • chemistry -

    convert Ea into kj

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