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Question
A reaction occurs in the following steps:
Step 1: \[\ce{NO_{2(g)} + F_2 -> NO2F_{(g)} + F_{(g)}}\] (slow)
Step 2: \[\ce{F_{(g)} + NO_{2(g)} -> NO_2F}\] (Fast)
- Write the equation of overall reaction.
- Write the rate law.
- Identify reaction intermediate.
Solution
- Overall reaction: \[\ce{2NO_{2(g)} + F_{2(g)} -> 2NO2F_{(g)}}\]
- Step 1 is slow. The rate law of the reaction is predicted from its stoichiometry. Thus, rate = k[NO2] [F2]
- F is produced in step 1 and consumed in step 2. Hence, F is the reaction intermediate.
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