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The following reaction is first order and the rate constant is 2.35 x 10^-4 s^-1 at 20 degress C.
2 N2O5 -----> 2 N2O4 + O2

A.) What is the rate of reaction if the [N2O5]=.25 M?




B. What would the [N2O5] be after 100 s given that the initial [N2O5] was 0.25 M? What would be the [N2O4]


C. What is the half life for this reaction?


D. How long will it take for the initial [N2O5]=0.88M to drop to 0.11 M?


E) What is the activation energy for the reaction if the rate constant at 30 degrees C is 9.15 x 10^-4 s^-1

F.) What is the rate constant at 70 degrees C?



I'm confused on how to solve these and I have to show work. This is a sample problem for me to work on also all the C have to be changed by adding 273. If someone can show the work and how to get through this it would be very helpful! Thanks!

  • Chemistry -

    The following reaction is first order and the rate constant is 2.35 x 10^-4 s^-1 at 20 degress C.
    2 N2O5 -----> 2 N2O4 + O2

    A.) What is the rate of reaction if the [N2O5]=.25 M?

    rate = k[N2O5]

    B. What would the [N2O5] be after 100 s given that the initial [N2O5] was 0.25 M? What would be the [N2O4]

    ln(Ao/A) = akt

    C. What is the half life for this reaction?

    k = 0.693/t1/2

    D. How long will it take for the initial [N2O5]=0.88M to drop to 0.11 M?
    ln(Ao/A) = akt

    E) What is the activation energy for the reaction if the rate constant at 30 degrees C is 9.15 x 10^-4 s^-1

    Use the Arrhenius equation.

    F.) What is the rate constant at 70 degrees C?
    Use the Arrhenius equation.

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