Reaction = 2H2 + 2NO --> 2H2O + N2
The rate = k[H2][NO]^2
I got:
Step 1: H2+2NO --> H2O2 + N2 (SLOW)
Step 2: H2O2 + H2 --> 2H2O (FAST)
The rate = k[H2][NO]^2
I got:
Step 1: H2+2NO --> H2O2 + N2 (SLOW)
Step 2: H2O2 + H2 --> 2H2O (FAST)
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LOL, you twit. This will get you lots of help: "Come on you dumb people, help me with this!!!"
2H2 + 2NO --> 2H2O + N2 ........... rate = k[H2][NO]^2
Why would you suggest H2O2 when the •OH radical will do? There are problems with suggesting a mechanism that requires three particles to collide simultaneously.
This mechanism is consistent with your rate law and does not require a reaction with a molecularity of 3.
NO + NO <==> N2O2.............. fast equilibrium
N2O2 + H2 --> N2O + H2O .....slow
N2O + H2 --> N2 + H2O ..........fast
-------------------------------------
2H2 + 2NO --> 2H2O + N2
2H2 + 2NO --> 2H2O + N2 ........... rate = k[H2][NO]^2
Why would you suggest H2O2 when the •OH radical will do? There are problems with suggesting a mechanism that requires three particles to collide simultaneously.
This mechanism is consistent with your rate law and does not require a reaction with a molecularity of 3.
NO + NO <==> N2O2.............. fast equilibrium
N2O2 + H2 --> N2O + H2O .....slow
N2O + H2 --> N2 + H2O ..........fast
-------------------------------------
2H2 + 2NO --> 2H2O + N2