KINETICS AND EQUILIBRIUM Calculating the reaction rate of one reactant from that

Question

KINETICS AND EQUILIBRIUM Calculating the reaction rate of one reactant from that of 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 860. liters per second of dioxygen are consumed when the reaction is run at 242. °C and 0.61 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 10 Explanation

Explanation / Answer

4NH3(g) + 5O2(g) = 4NO(g) + 6H2O(l)

Volume Of O2, V = 860 L/s

Temperature T = 242 + 273 = 515 K

P O2 = 0.61 atm

PV = nRT

n = PV/RT

= 0.61*860/0.0821*515

= 12.41 mol/s

Moles of NO produced = (4*12.41)/5 = 9.93 mol/s NO

Rate of NO produced = 9.93 mol/s x 30 g/mol

= 297.78 g/s

= 0.297 kg/s

= 2.97*10^-1 kg/s

Or

3.0 x 10^-1 kg/s

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