[TheBQ]

Hello all,

I've got a question from university about the production of nitric acid.

"Calculate the mass of 55% nitric acid solution produced in one ton of ammonia, if the percent yield of The oxidation of ammonia in the reactor is equal to 98% (step 1) and the production percent yield of the nitric acid is 94%."

Now I calculated and balanced the reaction and they are:

1. 2NO(g) + O₂(g)  2NO₂(g)
2. 2NO₂(g)    N₂O₄(g)
3. 3N₂O₄(g) + 2H₂O(l)  4HNO₃(aq) + 2NO(g)

So now I don't really know how to procced...

If any of you could help that would be a bless!

Thanks in advance.

[Borek]

Assuming 100% yield, how many moles of HNO₃ can be produced from one mole of NH₃?

[TheBQ]

Assuming 100% yield, how many moles of HNO₃ can be produced from one mole of NH₃?

That's my point I don't really know how to procced....

[Borek]

Follow atoms: if one molecule of ammonia contains one nitrogen atom, how many molecules of nitric acid can you produce?

And from one  mole?

[Q]

Assuming 100% yield, how many moles of HNO₃ can be produced from one mole of NH₃?

That's my point I don't really know how to proceed...

Ostwald process (the reaction):  NH₃(g) + 2O₂  HNO₃(aq) + H₂O(l) (ΔH=-370,3 kJmol^-1)

If the yield was 100% (η(reaction)=100%):
n(NH₃):n(HNO₃)=ν(NH₃):ν(HNO₃) => n(NH₃)=n(HNO₃)

The stoichiometric coefficient, ν, is the number written in front of atoms, ions, and molecules in a chemical reaction to balance the number of each element on both the reactant and product sides of the equation.