A two-step chemical reaction takes place with through the following mechanism:
Step 1: NO(g) + Br2(g) ↔ NOBr2(g) (fast)
Step 2: NOBr2(g) + NO(g) → 2 NOBr (g) (slow)
The proposed rate law for the overall reaction is: rate = k[NO][Br2]
A. Write the equation for the overall reaction, including states of matter.
B. Identify a catalyst (if possible).
C. Identify any/all intermediates (if possible).
D. Is this two-step mechanism consistent with the proposed rate law above? Show any/all substitution
steps if needed.
Answers: 1
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A two-step chemical reaction takes place with through the following mechanism:
Step 1: NO(g) + Br2(...
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