A proposed mechanism for the reduction of nitrogen as NO by hydrogen is: Step 1: H₂(g) + 2 NO(g) $\to$ N₂O(g) + H₂O(g) (slow)
Step 2: N₂O(g) + H₂(g) $\to$ N₂(g) + H₂O(g) (fast)
What is the rate law for step 2?

Question

A proposed mechanism for the reduction of nitrogen as NO by hydrogen is: Step 1: H₂(g) + 2 NO(g)

\to

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

\to

N₂(g) + H₂O(g) (fast)
What is the rate law for step 2?

Quizplus · Accepted Answer

The rate law for a reaction is determined by the slowest step, which in this case is step 1. Therefore, the concentration of H₂ is already taken into account in the rate law for step 1, and we only need to consider the concentrations of N₂O and H₂ for step 2. The rate law for step 2 is therefore k[H₂][N₂O].

A Proposed Mechanism for the Reduction of Nitrogen as NO →\to→

A Proposed Mechanism for the Reduction of Nitrogen as NO $\to$