Nitric acid is a key industrial chemical, largely used to make fertilizers and e

Question

Nitric acid is a key industrial chemical, largely used to make fertilizers and explosives. The first step in its synthesis is the oxidation of ammonia. In this reaction, gaseous ammonia reacts with dioxygen gas to produce nitrogen monoxide gas and wateir. Suppose a chemical engineer studying a new catalyst for the oxidation of ammonia reaction finds that 885. liters per second of dioxygen are consumed when the reaction is run at 225. °C and 0.97 atm. Calculate the rate at which nitrogen monoxide is being produced. Give your answer in kilograms per second. Round your answer to 2 significant digits. kg D-10

Explanation / Answer

225 degrees Celsius = 498.15 K

0.93 atm = 98. 28 kPa

Ideal gas law,

PV=nRT

n = ( 98.28 kPa *885) / (8.314 *103 L P / k mol) (498.15k)
n= 0.021 kmol.

= 21.00 gr-moles of Nitrogen produced.

0.021 kmol/second of O2 are produced.

But the reaction, stoichiometrically, is

4NH3+5O2 --> 4NO + 6H2O

5 moles of oxygen produce = 4 moles of NO

0.021 kmoles of oxygen produce = ( 4/5) * 0.021 NO

= 0.0168 kmol/s of NO

Molar mass of NO= 14+16=30.

Weight produced /s= molar mass * number of moles

= 30 gmol-1* 0.0168 kmol/s

= 0.5 kg /s

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