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 549 the reaction is run at 211. C and 0.96 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. liters per second of dioxygen are consumed when MacBook Air 1 6

Explanation / Answer

The balanced reaction is

4 NH3 + 5 O2 = 4 NO + 6 H2O

Volume of O2 consumed = 549 L/s

Temperature T = 211 + 273 = 484 K

Pressure P = 0.96 atm

Gas constant R = 0.0821 L-atm/mol-K

From the ideal gas equation

Moles of O2 consumed

n = PV/RT

= 0.96 atm x 549 L/s / 0.0821 L-atm/mol-K x 484 K

= 13.263 mol/s

Moles of NO produced

= 4 mol NO x 13.263 mol/s O2 / 5 mol O2

= 10.61 mol/s NO

Mass of NO produced = moles x molecular weight

= 10.61 mol/s x 30 g/nol

= 318.32 g/s x 1kg/1000g

= 0.318 kg/s

= 3.18 x 10^-1 kg/s

Related Questions

Navigate

• Browse (All)
• Browse N
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.