AIC600473Tribromamine decomposes to give nitrogen gas and hypobromous acid accordng to the overall reaction 2NBr3 + 3 0 H --N2 + 3Br-+ 3HOBr. Decomposition rates were measured over the p H range 6.00 f 0.05 to 8.00 i 0.05 for initial bromine to ammonia molar ratios between 4.00 and 12.0. The experimental rate law was found to be -d[NBr3]/dt = k,[NBr3]2[OH-]/[HOBr] + kb[NBr?]*, where k, = 1.07 X lo4 and kb = 0.34 I./(mol s) a t 20 "C. The first term in the rate equation is consistent with a mechanism in which the rate-determining step is preceded by equilibria among NBr3, NHBrz, HOBr, NBr2-, and OH-. Hydroxide may attack either NBr3 or NHBrz to produce NBr2-which subsequently reacts with NBr3. The second term is a simple second-order alternate pathway, occurring in acid solutions.

NBr3 zersetzt sich in wäßriger Lösung gemäß Gleichung A (Geschwindigkeitsgesetz und Konstanten bei 20°C).

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