First determine the formal oxidation numbers: N changes from +2 to +5 going from NO to (NO3)- O remains -2 the whole time Cr changes from +6 to +3 Now write the half reactions, balance the oxygens with the required number of waters and then balance the hydrogens with the required number of protons: Oxidation half reaction: NO(aq) + 2 H2O(l) ---> (NO3)-(aq) + 4 H+(aq) + 3 e- Reduction half reaction: (Cr2O7)2-(aq) + 14 H+(aq) + 6 e- ---> 2 Cr3+(aq) + 7 H2O(l) Now balance the number of electrons on both sides and add them together: 2 NO(aq) + 4 H2O(l) ---> 2 (NO3)-(aq) + 8 H+(aq) + 6 e- (Cr2O7)2-(aq) + 14 H+(aq) + 6 e- ---> 2 Cr3+(aq) + 7 H2O(l) --------------------------------------... 2 NO(aq) + (Cr2O7)2-(aq) + 6 H+(aq) ---> 2 (NO3)-(aq) + 2 Cr3+(aq) + 3 H2O(l) Notice that the charge is the same in both sides, which is an indication that the redox equation has been balanced correctly: -2 + 6 = -2 + 2(+3) +4 = +4
