The experimentally determined rate law for the reaction �
H2 + NO --> ½N2 + H2O is Rate = k[H2][NO]2. �
Is the mechanism below possible?�
Step 1: H2 + NO --> N + H2O Slow�
Step 2: N + NO -->N2 + O Fast�
Step 3: O + H2 --> H2O Fast
1. Yes, because the slow step reactants are the same as the overall reaction
2.Yes, because it is consistent with the rate law.
3.No, because it is not consistent with the rate law
I was thinking that the answer was #2, but Im not exactly sure why!
The answer is indeed option #1: "Yes, because the slow step reactants are the same as the overall reaction."
To determine if a proposed mechanism is possible, we need to check if it matches the overall balanced equation and if the rate law is consistent with the proposed mechanism.
In this case, the overall balanced equation is: H2 + NO --> ½N2 + H2O. Looking at the proposed mechanism:
Step 1: H2 + NO --> N + H2O (Slow)
Step 2: N + NO --> N2 + O (Fast)
Step 3: O + H2 --> H2O (Fast)
From the balanced equation, we can see that the reactants for the overall reaction are H2 and NO, which are also the reactants for the slow step in the proposed mechanism. This indicates that the proposed mechanism is consistent with the overall reaction.
Therefore, the answer is option #1, because the slow step reactants in the proposed mechanism are the same as the reactants in the overall reaction.