The decomposition of nitramide, O_2NNH_2, in water has the following chemical eq

Question

The decomposition of nitramide, O_2NNH_2, in water has the following chemical equation and rate law. O_2NNH_2 (aq) rightarrow N_2O(g) + H_2O (l) rate = k [O_2NNH_2]/[H^+] A proposed mechanism for this reaction is O_2NNH_2(aq) rightharpoonoverleftharpoon^k_1_k_-1 O_2NNH^-(aq) + H^+(aq) (fast equilibrium) O_2NNH_2(aq) rightarrow k_2 N_2O(g) + OH^-(aq) (slow) H^+(aq) + OH^-(aq) rightarrow^k_3 H_2O(l) (fast) Determine the law for each elementary step. Drag the symbols into the equations as needed. rate_1 = k_1 [O_2NNH_2] [N_2O] rate_1 = k_1 [O_2 NNH^-] k_2 [H^+] rate_2 = k_3 [OH^-] rate_3 = [H_2O] Which of these rates is equal to the overall reaction rate? rate_1 rate_-1 rate_2 rate_3

Explanation / Answer

Rate= K3[O2NNH-]   (1)

the term of O2NNH- is intermediate that needs to be eliminated.

Since 1st step of the mechanism is at equilibrium

K1[O2NNH2]=K2[O2NNH-][H+]

[O2NNH-] = (K1/K2) [O2NNH2]/[H+] = K [O2NNH2]/[H+], where K is constant.

Hence Eq.1 becomes rate= K3K[O2NNH2]/[H+]

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