How to balance this redox equation? PLEASE HELP!!!

For the equation Ag + NO3 -  Ag + + NO
(Note: This reaction takes place in an acidic solution.)

Step 1: What substance is reduced?

Step 2: What substance is oxidized?

Step 3: What is the half reaction for oxidation?

Step 4: What is the half reaction for reduction?

Step 5: What is the net balanced equation?

Step 6: What is the reduced equation?


This is what I got, please tell me what I did wrong, b/c my teacher graded this question and it was incorrect.


Step 1
NO3 -
Step 2
Ag
Step 3
Ag Ag+e-
Step 4
NO3 - + 3 e NO
Step 5:
3Ag(s) + NO3- + 4H+ --> 3Ag+ + NO(g) + 2H2O(l)
Step 6
3Ag(s) + NO3- + 4H+ --> 3Ag+ + NO(g) + 2H2O(l)

Your steps 1, 2 and 3 all look correct to me.

For step 4, you should have a balanced half-reaction which would be:

NO3- + 4 H+ + 3 e- --> NO + 2 H2O

I don't know the distinction between "net balanced equation" and the "reduced equation". I think those are correct. You might ask your teacher what he/she meant for you to put for those...