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### Topic: Production of Nitric Acid  (Read 1242 times)

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#### TheBQ

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• Mole Snacks: +0/-0 ##### Production of Nitric Acid
« on: July 08, 2021, 02:24:49 PM »
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!

« Last Edit: July 08, 2021, 04:54:44 PM by sjb »

#### Borek ##### Re: Production of Nitric Acid
« Reply #1 on: July 08, 2021, 02:26:38 PM »
Assuming 100% yield, how many moles of HNO3 can be produced from one mole of NH3?
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#### TheBQ

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• Mole Snacks: +0/-0 ##### Re: Production of Nitric Acid
« Reply #2 on: July 08, 2021, 02:35:40 PM »
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 ##### Re: Production of Nitric Acid
« Reply #3 on: July 08, 2021, 03:02:11 PM »
Follow atoms: if one molecule of ammonia contains one nitrogen atom, how many molecules of nitric acid can you produce?

And from one  mole?
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#### Q

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« Reply #4 on: July 18, 2021, 10:25:01 AM »
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.