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 water. Suppose a chemical engineer studying a new catalyst for the oxidation of ammonia reaction finds that 714. liters per second of dioxygen are consumed when the reaction is run at 211. oC and 0.98 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

Explanation / Answer

1)

First we have to calculate the moles of oxygen.

Given that

volume of oxygen   V = 714 L

Temp T = 211 oC = 211 + 273 K = 484 K

Pressure P = 0.98 atm

moles of oxygen n = ?

Ideal gas equation is PV=nRT   , R = 0.0821 L.atm/K/mol

n = PV/RT

= (0.98 atm x 714 L) / (0.0821 L.atm/K/mol x 484 K)

= 17.6 moles

= 0.0176 kmol

n = 0.0176 kmol

Hence,

0.0176 kmol of O2 is consumed per second.

But the balanced equation for oxidation of NH3 is

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

             5 mol                4 mol

             0.005 kmol        4 x 30 = 120 g = 0.120 kg     [ molar mass of NO = 30 g/mol]

            0.0176 kmol           ?

? = (0.0176 kmol O2/ 0.005 kmol O2) x 0.120 kg

     = 0.4224 kg

Therefore,

rate at which Nitrogen monoxide (NO)produced   = 0.4224 kg/s

Ans = 0.4224 kg/s

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