he decomposition of nitramide, O2NNH2, in water has the following chemical equat

Question

he decomposition of nitramide, O2NNH2, in water has the following chemical equation and rate law. O2NNH2 (aq) yields N2O (g) + H2O (l) rate= [O2NNH2]/[H]

A proposed mechanism for this reaction is.

k1

(1) O2NNH2 (aq) equilibrium O2NNH (aq) + H (aq) (fast equilibrium)

k-1

k2

(2) O2NNH (aq) yields N2O (g) + OH (aq) (slow)

k3

(3) H (aq) + OH yields H2O (l) (fast)

What is the relationship between the observed value of k and the rate constants for the individual

steps of the mechanism?

k=__________

Also which symbols go into the numerator or demoniator k-1, k3, k2, k1

Explanation / Answer

For my convenience I denote O?NNH? with N and O? NN H- with I (intermediate). Then r = k[I]. From the equilibrium one gets K= k1/k-1= [I][H+]/[N]. Solve for [I] and insert in to rate law: r= k2 k1 [N]/ ( k-1 [H+] ) and by comparison: k= k1 k2/k-1

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