The first step in the synthetic manufacture of nitric acid is the oxidation of a

Question

The first step in the synthetic manufacture of nitric acid is the oxidation of ammonia to nitric oxide. (NH_3 reacts with O_2 to form NO and H_2O). The commercial procedure is to feed the ammonia vapor at 25 degree C into stream of air at 700 degree C before it passes over the catalyst. Sufficient air is used to provide 10% excess over that needed to oxidize all the ammonia. Approximately 80% of the NH_3 is oxidized to NO, and the gases leave at the reaction temperature of 920 degree C. Using a basis of 4 gmol of NH_3: (a) Write the balanced chemical reaction equation for the oxidation of ammonia with stoichiometric oxygen. (b) Write the balanced chemical reaction equation for the oxidation of ammonia using with 10% excess air and complete 100% oxidation of the NH_3. (c) Write the balanced chemical reaction equation for the oxidation of ammonia using with 10% excess air and partial 80% oxidation of the NH_3. (d) Assume that 4 gmol/min of NH_3 are fed to the reactor, calculate the gmols of all compounds entering and leaving the reactor. (e) Using the basis of the elements at 25 degree C and 1 atm, calculate the enthalpy (kJ/gmol) of all compounds entering and leaving the reactor and the overall heat flow to or from the reactor. For simplicity, assume and use the following average (and constant) specific heats: (f) To check your work complete the following Table.

Explanation / Answer

(a) Ammonia NH3 reacts with O2 to give NO and and H2O

So, Balancing this, NH3 + O2 ==> NO + H2O

Balance Hydrogen,

4 NH3 + O2 = NO + 6 H2O

Now, balance N,

4 NH3 + O2 = 4 NO + 6 H2O

Now, balance O,

4 NH3 + 5 O2 = 4 NO + 6 H2O

Hence, the balanced equation.

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