As a first step in the production of nitric acid, ammonia is oxidized to form nitric oxide: 4NH3 + 5O2→4NO + 6H2O
A side reaction also occurs:
2NH3 +3/2O2→N2 +3H2O
A reactor is designed to carry out this reaction isothermally at 600°C, with pure oxygen fed to the reactor in 50% excess. At these conditions, all components are in the gas phase. The conversion of ammonia is 80%, and the selectivity ratio of NO to N2 in the product stream is 15:1. The reactor products are fed to a separator where 75% of the NH3 and O2 are recycled and combined with a fresh feed. The remainder of the reactor products are removed as a product. Assume a feed flowrate of 2100 SLPM of ammonia. (25 points)
Determine the flow rate, in moles per second, of all the products leaving the reactor.
Determine the flowrate and composition of the fresh feed in moles per second.
I have assumed that the given conversion is the overall conversion which is defined as the ratio of moles of NH3 reacted overall to the moles of NH3 fed into the system.
The required material balances with the use of stoichiometry is shown below.
As a first step in the production of nitric acid, ammonia is oxidized to form nitric...
An Important step in the synthesis of nitric acid is the conversion of ammonia to nitric oxide according to the following balanced chemical equation. What is AHpxn for this reaction? 4NH3(g) + 5O2(g) -4NO(g) + 6H2O(9) Substance AH?f(kJ/mol) NH3(g) -46.3 NO(9) 90.3 H2O(9) -241.8 0 -1274.8 kJ/mol -904.4 kJ/mol 0 -240.2 kJ/mol 0 -197.8kJ 197.8 kJ/mol
Ammonia reacts with oxygen to form nitric oxide and water vapor: 4NH3 +5O2 → 4NO + 6H2O What is the theoretical yield of water, in moles, when 40.0g NH3 and 50.0g O2 are mixed and allowed to react: 1.87 mol 3.53 mol 1.57 mol 1.30 mol None of these
The first step in the Ostwald process for making nitric acid is the formation of NO as follows: 4NH3 + 5O2 => 4NO + 6H2O According to the equation, 5 moles of NH3 will react stoichiometrically with ________ moles of O2 to form _______ moles of NO. A. 4, 5 B. 5, 4 C. 25, 20 D. 5/4, 4/5 E. 25/4, 5
One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3 to NO: 4NH3(g)+5O2(g)→4NO(g)+6H2O(g) In a certain experiment, 2.05 g of NH3 reacts with 3.76 g of O2. How many grams of NO and of H2O form? Enter your answers numerically separated by a comma.
The first step in industrial nitric acid production is the catalyzed oxidation of ammonia. Without a catalyst, a different reaction predominates: 4NH3(g) + 3O2(g) ⇔ 2N2(g) + 6H2O(g) When 0.0160 mol gaseous NH3 and 0.0220 mol gaseous O2 are placed in a 1.00 L container at a certain temperature, the N2 concentration at equilibrium is 2.70×10-3 M. Calculate Keq for the reaction at this temperature.
One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3 to NO: 4NH3(g)+5O2(g)→4NO(g)+6H2O(g) In a certain experiment, 1.85 g of NH3 reacts with 3.39 g of O2. 1) How many grams of NO and of H2O form? 2) How many grams of the excess reactant remain after the limiting reactant is completely consumed?
Ammonia reacts with oxygen to form nitric oxide and water vapor: 4NH3 + 5O2 ---> 4NO + 6H2O When 20.0 g NH3 and 50.0 g O2 are allowed to react, which is the limiting reagent? A) NO B) O2 C) H2O D) no reagent is limiting E) NH3 What is the coefficient for O2 when the following combustion reaction of a hydrocarbon is balanced? ___C7H14 + ___ O2 ---> ___ CO2 + __ H2O A) none of these B) 10...
Nitric oxide (NO) can be produced by partially oxidizing ammonia (NH3) with oxygen via the following reaction: 2NH3 + 2.5O2 = 2NO + 3H2O (1) Ammonia can also react with oxygen via the following reactions: 2NH3 + 1.5O2 = N2 + 3H2O (2) 2NH3 + 3.5O2 = 2NO2 + 3H2O (3) Ammonia is fed to a reactor at 25 °C and 500 kg/h. Dry air (21 mol % O2, 79 mol % N2) enters at 8000 kg/h. Eighty percent (80%)...
Always show your work. No credit will be given for any answers (even if they are correct) for which work is not shown. Ammonia reacts with diatomic oxygen to form nitric oxide and water vapor: 4NH3 + 502 ---> 4NO + 6H2O What is the theoretical yield of water, in moles, when 40.0 g NH3 and 50.0g, O2 are mixed and allowed to react?
The first step in the Oswald process for producing nitric acid is 4NH+5o2- 4NO + 6H2O if 132g of ammonia reacts with 132g of oxygen A) how many grams of nk itric oxide(No) will be produced B) which compound is limiting reagent C) what is the % yield of this reaction if actual yield of NO is 67.Og?