The first order rate constant for the decomposition of N_2O_5 is 6.2 times 10^-4

Question

The first order rate constant for the decomposition of N_2O_5 is 6.2 times 10^-4 at 45.0degreeC and 2.1 times 10^-3 at 55.0degreeC. Determine the magnitude of the pre-exponential factor, A, for this reaction. This term includes the frequency factor and the orientation factor. The Arrhenius equation is: k=Ae^-Ea/RT which can be re-written as: ln(k_2/k_1) = (E_a/R) ((1/T_1) - (1/T_2)) or ln(k) =-(E_a/R)(l/T) + In A You will first need to solve for the Activation energy, E_a The Arrhenius factor, A =

Explanation / Answer

ln((2.1*10^-3)/(6.2*10^-4)) = (x/8.314)((1/318.15)-(1/328.15))

Ea = 1.06*10^2 kj

ln(2.1*10^-3) = -(1.06*10^5/8.314)(1/328.15)+ln(A)

A = 1.57*10^14

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