Originally posted by dannyUchiha
How do you propose the reaction would occur?
I know that nitric acid rarely produces hydrogen when it reacts with metals (excpet for magnesium and calcium,when cold and dilute)
In reality the products you obtain usually depends on the temperature and the concentration of the acid used.
A common reaction is copper with conc.nitric acid
Cu + 4HNO3 -> Cu(NO3)2 + 2NO2 + 2H2O
However I think this is only for metals low in the electrochemical series (e.g. Cu & Pb).
However becuase sodium is such a good reducing agent, maybe it will reduce the N further, here are the possible options. I would imagine you need to look at the standard reduction potentials.
1. Na + 2HNO3 -> NaNO3 + NO2 + H2O
(Here nitrate reduced from +5 to +4 in nitrogen dioxide)
2. 3Na + 4HNO3 -> 3NaNO3 + NO + 2H2O
(Here nitrate reduced from +5 to + 2 in nitrogen monoxide)
3. 8Na + 10HNO3 -> 8NaNO3 + 5H2O + N2O
(here nitrate reduced from +5 to +1 in dinitrogen oxide)
4. 6Na + 8HNO3 -> 6NaNO3 + 2H2O + NH3OHNO3
(Here the nitrate reduced from +5 to -1 in hydroxylammoniumn ions)
5. 8Na + 10HNO3 -> 8NaNO3 + NH4NO3 + 3H2O
(Here the nitrate reduced from +5 to -3 in ammonium ions)
Trust me you wont find this in any books or anywhere on the internet, that is why I asked the question!
It's all self worked out 😉
My gut feeling is number 5 😉