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Production of Nitric Acid

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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)  ::equil:: 2NO2(g)
2. 2NO2(g)   ::equil:: N2O4(g)
3. 3N2O4(g) + 2H2O(l)  ::equil:: 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!

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

TheBQ:

--- Quote from: Borek on July 08, 2021, 02:26:38 PM ---Assuming 100% yield, how many moles of HNO3 can be produced from one mole of NH3?

--- End quote ---

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:

--- Quote from: TheBQ on July 08, 2021, 02:35:40 PM ---
--- Quote from: Borek on July 08, 2021, 02:26:38 PM ---Assuming 100% yield, how many moles of HNO3 can be produced from one mole of NH3?

--- End quote ---

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

--- End quote ---

Ostwald process (the reaction):  NH3(g) + 2O2  :rarrow: 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.