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Question
The reaction \[\ce{2NO2Cl_{(g)} -> 2NO2_{(g)} + Cl2_{(g)}}\] takes place in two steps as
(i) \[\ce{NO2Cl_{(g)} -> NO2_{(g)} + Cl_{(g)}}\]
(ii) \[\ce{NO2Cl_{(g)} + Cl_{(g)} -> NO2_{(g)} + Cl2_{(g)}}\]
Identify the reaction intermediate.
Options
NO2(g)
NO2Cl(g)
Cl(g)
Cl2(g)
MCQ
Solution
Cl(g)
Explanation:
\[\ce{NO2Cl_{(g)} ->[R.D.S.] NO2_{(g)} + Cl_{(g)}}\] ..........(1)
\[\ce{NO2Cl_{(g)} + Cl_{(g)} -> NO2_{(g)} + Cl2_{(g)}}\] .......(2)
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\[\ce{2NO2Cl_{(g)} -> 2NO2_{(g)} + Cl2_{(g)}}\]
Rate = k[NO2Cl]
The reaction intermediate is formed and gets consumed in the reaction.
Reaction intermediate = Cl(g)
shaalaa.com
Molecularity of Elementary Reactions
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