In this question, I couldn't reconcile with the answer.
1. Step 3 is slowest
2. So rate law = k [NO+] [ NH3]
3. But we cannot have a rate law in terms of intermediates
4. NH3 is intermediate. So per rate law of step 2, R = k[NH4+]
5. So overall rate law is R = k[NO+] [NH4+]
Please explain the logic of your answer and where am I wrong
Overall reaction is
HNO2 + NH4+ ...> 2H2O +N2
Rate law for step I
Rate = k[HNO2][H+]
Rate law for step 2
Rate = k[NH4+]
step 3
Rate =k[NO+][NH3]
This step is rate law determining step and you need to remove intermediate by reactants from which these intermediates are formed.
Replace NO+ by HNO2 and H+
Replace NH3 by NH4+
Here H+ is the catalyst.