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 oxidiation 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 reactions finds that 613. liters per second of dioxygen are consumed when the reaction is run at 175. C and 0.16 atn=m. Calculate the rate at which nitrogen monoxide is being produced. Give your answer in Kg/second. Round your answer to 2 significant digits.

Explanation / Answer

the reaction is as follows

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

So, rate of consumption of O2 = rate of production of NO

-5 d[O2]/dT = +4 d[NO]/dT

5 * 613 = 4d[NO]/dT

  d[NO]/dT= (5*613)/4

= 766,25 L/ s

to convert into Kg/ s we need density of NO which is 1.34 kg/m3 = 1.34 * 10-3kg/L

mass= Vol * density

= 766.25 * 1.34 * 10-3

= 1.026 kg

therefore rate is 1.03Kg/second for NO in two significant figures

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