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The reaction for the decomposition of dinitrogen monoxide gas to form an oxygen radical is: N2O(g)==>N2(g)+O(g) . If the activation energy is 250 kJ/mol and the frequency factor is 8.0 x 1011 s-1, what is the rate constant for the first-order reaction at 1000 K?

k = A * exp ( -Ea / RT )

k = rate constant (s-1)
A = frequency factor or preexponential factor (s-1)
Ea = activation energy (J / mol)
R = gas constant (J / K*mol)
T = Temp (K)


did i set this up right?

  • Chemistry - ,

    Never mind i know i didn't what goes in the exp?

  • Chemistry - ,

    I use it in the form that follows:
    ln(k2/k1) = Ea/R(1/T1 - 1/T2)
    You must insert A appropriately.

  • Chemistry - ,

    i don't understand where k1 k2 t1 t2 come from... :(

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