Ammonia is oxidized to nitric oxide in the following reaction: 4NH_3 + 5O_2 righ

Question

Ammonia is oxidized to nitric oxide in the following reaction: 4NH_3 + 5O_2 rightarrow 4NO + 6 H_2O NH_2, O_2, and H_2O enter the reactor in the feed stream. The product stream leaving the reactor has a flow rate of 100 mole/s, containing 10 mol% NH_3, 10 mole % O_2, 20% NO, and 60% H_2O. Calculate the flow rates of each of the chemicals in the feed stream: NH_3 _____ mole/s: Q_2 _____ mole/s; H_2O _____ mole/s Calculate the fractional conversion of: NH_3 _____ Which chemical is the excess reactant? _____ What is the % excess of the excess reactant?

Explanation / Answer

Product stream flow rate = 100 mol/s

Flowrate of NO = 0.20 x 100 mol/s = 20 mol/s

NH3 and NO mole ratio = 4:4 = 1:1

This means 20 mol/s of NH3 is reacted .

NH3 and O2 mole ratio = 4:5

Moles rate of O2 reacted = (5/4) x 20 = 25 mol/s

NH3 and H2O mole ratio = 4:6 = 2:3

Moles rate of H2O formed = (3/2) x 20 = 30 mol/s

Now to find initial moles, we add mol/s of species reacted + mol/s of species left.

Initial mol/s of NH3 = 20 + 10 = 30 mol/s

Initial mol/s of O2 = 25 + 10 = 35 mol/s

Initial mol/s of H2O = 60 - 30 = 30 mol/s

(b) fractional conversion of NH3 = moles reacted / moles fed = 20/30 = 0.67

(c) 1 mol NH3 requires 1.25 mol O2

so 20 mol/s of NH3 requires , 20 x 1.25 = 25 mol/s but we have 30 mol/s

so excess reactant is O2

% excess = (30-25) / 25 x 100 = 20%

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