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11 Dec 2019

Nitric acid (HNO3), a strong acid, is formed in the following reaction.

2 NO(g) + 3/2 O2(g) + H2O(g) → 2 HNO3(g).

Assume a volume of 22.4 mL of NO gas (at STP = 1 atm, 273 K) completely reacts with
excess of oxygen and water. If all of the acid that is formed is dissolved into 50. mL of
water, what should be the pH of the solution? (pH = - log[H+])?
A) 1.0
B) 1.7
C) 2.0
D) 3.0
E) 2.3

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Trinidad Tremblay
Trinidad TremblayLv2
13 Dec 2019

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Related questions

The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (O2) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here: ?NH3(g)+?O2(g)→?NO(g)+?H2O(g) What volume of O2 at 684 mmHg and 27 ∘C is required to synthesize 20.0 mol of NO?

Nitric acid may be produced by oxidizing ammonia to nitric oxide over a platinum-rhodium catalyst, then oxidizing the nitric oxide to nitrogen dioxide in a separate unit where it is absorbed in water to form an aqueous solution of nitric acid. The three key reactions in the synthesis are the oxidation of the ammonia to nitric oxide and of nitric oxide to nitrogen dioxide, followed by dissolution of the NO2 in water:

4NH3(g)+ 5O2(g)→ 4NO(g)+ 6H2O(g)

2NO(g) + O2(g) → 2NO2(g)

4NO2 (g)+ 2H2O(l) + O2(g) → 4HNO3(aq)

In this problem, you may neglect side reactions that would lower the product yield. This would include the side reaction in which ammonia is oxidized to form nitrogen and water which can lower product yield.

4NH3 + 3O2 → 2N2 + 6H2O

Thus, for this project the overall reaction may be represented from the three key reactions above as:

NH3 + 2O2 → H2O + HNO3

Ammonia vapor at 275oC and 8 atm is mixed with air, also at 275oC and 8 atm, and the combined stream is fed to a converter. Fresh air entering the system at 30oC and 1 atm with a relative humidity of 50% is compressed to 100oC and 8 atm, and the compressed air then exchanges heat with the product gas leaving the converter. The quantity of oxygen in the feed to the converter is 20% in excess of the amount theoretically required to convert all the ammonia to HNO3. The entire process after the compressor may be taken to operate at a constant pressure of 8 atm.

In the converter, the ammonia is completely oxidized, with a negligible amount of NO2 formed. The product gas leaves the converter at 850oC and exchanges heat with the air leaving the system as described earlier. The product gas is then fed to a waste-heat boiler that produces superheated steam at 200oC and 10 bar from liquid water at 35oC. The product gas leaving the waste-heat boiler is cooled further to 35oC and fed to an absorption column in which the NO is completely oxidized to NO2 which in turn combines with water (some of which is present in the product gas). Water is fed to the absorber at 25oC, at a rate sufficient to form a 55 wt% aqueous nitric acid solution. Any NO formed in the reaction of NO2 to produce HNO3 is oxidized and the NO2 produced is hydrated to form still more HNO3. The off-gas from the process may be taken to contain only N2 and O2 and at 25oC and 1 atm.

b). Taking a basis of 100 kmol of ammonia fed to the process

(i) kmol of water fed to the absorber

(ii). Temperature of the product gas after it has exchanged heat with the air, assuming no heat is transferred between the heat exchanger and the surroundings

The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (O2) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here:

?NH3(g)+?O2(g)→?NO(g)+?H2O(g)

Part A

What volume of O2 at 836 mmHg and 27 ∘C is required to synthesize 10.5 mol of NO?

Express your answer to three significant figures and include the appropriate units.

Part B

What volume of H2O(g) is produced by the reaction under the same conditions?

Express your answer to three significant figures and include the appropriate units

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