Could someone out there please help me try and balance the following redox equation? I have all the reagents and products, but just need to balance them with stoichiometric coefficients.
[Co(NH3)5Cl]Cl2 + HNO3 ------> Co(NO3)2 + HCl + NO + H2O
I know that these are the following half reactions:
Co3+ ----> Co2+ + 1 electron
N(-3) ----> N(+2) + 5 electrons
But, both of these elements are in the complex, and since the number of electrons being reduced must equal the number of electrons oxidized, how can balance this if, there are 5 NH3 ligands in the complex (which would be 25 electrons transferred) and only 1 electron transferred per cobalt atom? Or do the other nitrogens somehow get involved?
If someone could please provide me with an explanation, that would be awesome. Thanks!