Nitric acid is manufactured in the Oswald process, which involves the catalytic

Question

Nitric acid is manufactured in the Oswald process, which involves the catalytic oxidation of ammonia according to the following equations: (i) 4 NH3(g) + 5 O2(g) 4 NO(g) + 6 H2O(g) (ii) 2 NO(g) + O2(g) 2 NO2(g); (iii) 3 NO2(g) + H2O(l) 2 HNO3(aq) + NO(g); How many gallons of 70.0% (by mass) of concentrated HNO3 solution (density = 1.48 g/mL) can be produced from 1.00 metric tonne (1.00 x 103 kg) of ammonia gas? Assume a 100% yield. (1 gall = 3.7854 L; 1 gallon of concentrated HNO3 weighs 5.60 kg)

Explanation / Answer

(i) 4 NH3(g) + 5 O2(g) 4 NO(g) + 6 H2O(g)

(ii) 2 NO(g) + O2(g) 2 NO2(g);

(iii) 3 NO2(g) + H2O(l) 2 HNO3(aq) + NO(g)

from... 1 metric ton = 10^3 kg = 10^6 g

mol = mass/mW = (10^6)/(17) = 58823.529 mol of NH3

so...

4 mol of NH3 --> 4 mol of NO --> 4 mol of NO2 --> 2.66 mol of HNO3

so

1 mol of NH3 = 2.66/4 mol of HNO3 = 0.665 mol of HNO3

so..

58823.529 mol of NH3 = 58823.529 *0.665 = 39117.64 mol of HNO3

so..

mass of HNO3 = mol*MW =39117.64*63.01 = 2464802.49 grams of HNO3 = 2.46*10^6 g of HNO3...

1 gal = 5.6 kg

x gal = 2464.80 kg

soo

x = 2464.80 /5.6 = 440.1428 gallons of concentrated acid (i.e. at 70%)

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