The reaction of NO gas with H₂ gas has the following rate law: Rate = k[H₂][NO]².A proposed mechanism is: Step 1: H₂(g) + 2 NO(g) $\to$ N₂O(g) + H₂O(g)
Step 2: N₂O(g) + H₂(g) $\to$ N₂(g) + H₂O(g)
What is the molecularity of steps 1 and 2,and which step is the rate-determining step?

Question

The reaction of NO gas with H₂ gas has the following rate law: Rate = k[H₂][NO]².A proposed mechanism is: Step 1: H₂(g) + 2 NO(g)

\to

N₂O(g) + H₂O(g)
Step 2: N₂O(g) + H₂(g)

\to

N₂(g) + H₂O(g)
What is the molecularity of steps 1 and 2,and which step is the rate-determining step?

Quizplus · Accepted Answer

Step 1 involves three molecules (1 H2 and 2 NO), making it termolecular. Step 2 involves two molecules (1 N2O and 1 H2), making it bimolecular. The rate law matches step 1, indicating it is the rate-determining step.

The Reaction of NO Gas with H2 Gas Has the Following

The Reaction of NO Gas with H₂ Gas Has the Following