The following are the steps to complete and balnce the equation for the given reaction
<u>Explanation:</u>
We are given, NO2– is oxidized to NO3– and Ag is reduced to Ag
NO2– + Ag+ -----> NO3– + Ag(s)
Step 1) Assign the oxidation state to each element reaction
NO2– + Ag+ -----> NO3– + Ag(s)
N= +3 N = +5
O = -2 O = -2
Ag = +1 Ag = 0
NO2– -----> NO3– ………oxidation half reaction
Ag+ -----> Ag(s) ……….reduction half reaction
Step 2) Balance the element other than O and H
NO2– -----> NO3–
Ag+ -----> Ag(s)
Step 3) Balance the O by adding 1 H2O for 1 O
NO2– + H2O -----> NO3–
Ag+ -----> Ag(s)
Step 4) Balance the H by adding H+
NO2– + H2O -----> NO3– + 2H+
Ag+ -----> Ag(s)
Step 5) Balance the charge by adding electron
NO2– + H2O -----> NO3– + 2H+ + 2e-
Ag+ + 1e------> Ag(s)
Step 6) Balance the electron in both half reaction
NO2– + H2O -----> NO3– + 2H+ + 2e-
2 Ag+ + 2e------> 2 Ag(s)
