Nitryl bromide, NO2Br, decomposes into nitrogen dioxide and bromine. 2NO2Br(g) ? 2NO2(g) + Br2(g) A proposed mechanism is NO2Br ? NO2 + Br (slow) NO2Br + Br ? NO2 + Br2 (fast) What is the rate law predicted by this mechanism?
Added by Sean H.
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The rate law for the slow step, which is the rate determining step, is rate = k[NO2Br]. Show more…
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David C.
Nitryl bromide, $\mathrm{NO}_{2} \mathrm{Br}$, decomposes into nitrogen dioxide and bromine. $$ 2 \mathrm{NO}_{2} \mathrm{Br}(g) \longrightarrow 2 \mathrm{NO}_{2}(g)+\mathrm{Br}_{2}(g) $$ A proposed mechanism is $$ \begin{array}{r} \mathrm{NO}_{2} \mathrm{Br} \longrightarrow \mathrm{NO}_{2}+\mathrm{Br} \\ \mathrm{NO}_{2} \mathrm{Br}+\mathrm{Br} \longrightarrow \mathrm{NO}_{2}+\mathrm{Br}_{2} \end{array} $$ Write the rate law predicted by this mechanism.
Consider the following three-step mechanism for a reaction: Br2 (g) ⇌ 2 Br (g) Fast Br (g) + CHBr3 (g) → HBr (g) + CBr3 (g) Slow Br (g) + CBr3 (g) → CBr4 (g) Fast Based on this mechanism, determine the rate law for the overall reaction. Consider the overall reaction: AB(g) + CB(g) ⟶ A(g) + CB2(g) A proposed mechanism for this reaction is: 2 AB(g) ⇌ AB2(g) + A(g) (fast) AB2(g) + CB(g) ⟶ AB(g) + CB2(g) (slow)
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