$A$ complex reaction takes place in the following steps:
$NO_2Cl_{(g)} \longrightarrow NO_{2(g)} + Cl_{(g)}$ (slow)
$NO_2Cl_{(g)} + Cl_{(g)} \longrightarrow NO_{2(g)} + Cl_{2(g)}$ (fast)
Identify the rate law equation for this reaction.
$NO_2Cl_{(g)} \longrightarrow NO_{2(g)} + Cl_{(g)}$ (slow)
$NO_2Cl_{(g)} + Cl_{(g)} \longrightarrow NO_{2(g)} + Cl_{2(g)}$ (fast)
Identify the rate law equation for this reaction.
- A$r = k[NO_2Cl]$
- B$r = k[NO_2][Cl]$
- C$r = k[NO_2]^2$
- D$r = k[NO_2Cl]^2$
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