For a reaction carried at 400 K, `NO_(2)(g) + CO_(2)(g) to CO_(2)(g) + NO_(2)(g)`, the proposed mechanism is as follows: `NO_(2) + NO_(2) overset("Slow")to NO + NO_(3) NO_(3) + CO overset("Fast")to CO_(2) + NO_(2)` What is the rate law for the reaction?

For a reaction carried at 400 K, `NO_(2)(g) + CO_(2)(g) to CO_(2)(g) +

1.	For a reaction carried at 400 K, `NO_(2)(g) + CO_(2)(g) to CO_(2)(g) + NO_(2)(g)`, the proposed mechanism is as follows: `NO_(2) + NO_(2) overset("Slow")to NO + NO_(3) NO_(3) + CO overset("Fast")to CO_(2) + NO_(2)` What is the rate law for the reaction?
Answer» The slow step for the reaction is: `NO_(2) + NO_(2) to NO + NO_(3)` (Slow) The rate law equation is: `Rate( r) = k[NO_(2)][NO_(2)]= k[NO_(2)]^(2)`.

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For a reaction carried at 400 K, `NO_(2)(g) + CO_(2)(g) to CO_(2)(g) + NO_(2)(g)`, the proposed mechanism is as follows: `NO_(2) + NO_(2) overset("Slow")to NO + NO_(3) NO_(3) + CO overset("Fast")to CO_(2) + NO_(2)` What is the rate law for the reaction?

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