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Nitric acid is produced commercially by a multi-step process, starting from the oxidation of ammonia. If...
The first step in industrial nitric acid (HNO3) production is the catalyzed oxidation of ammonia (NH3). Without the catalyst the following reaction predominates: 4NH3(g) + 3O2(g) ⇔ 2N2(g) + 6H2O(g). When 0.0150 mol each of NH3(g) and O2(g) are placed in a 1.00 L container at a certain temperature the N2(g) concentration at equilibrium is 1.96x10-3 M. Fill in the following ICE table and calculate the resulting KC. NH3(9) 02(9) N2(9) H20(9) Initial (1) 015 mol mol .015 Number Number...
The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in many modern chemical processes. In the first step of the Ostwald process, ammonia is reacted with oxygen gas to produce nitric oxide and water. What is the maximum mass of H2O that can produced by combining 67.5 g of each reactant? 4NH3(g)+5O2(g)-------- >4NO(g)+6H2O(g)
The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in many modern chemical processes. In the first step of the Ostwald process, ammonia is reacted with oxygen gas to produce nitric oxide and water. What is the maximum mass of H2OH2O that can be produced by combining 86.7 g86.7 g of each reactant? 4NH3(g)+5O2(g)⟶4NO(g)+6H2O(g)
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.
The commercial production of nitric acid involves the following chemical reactions: (a) 4NH3(g)+5O2(g)⟶4NO(g)+6H2O(g) (b) 2NO(g)+O2(g)⟶2NO2(g) (c) 3NO2(g)+H2O(l)⟶2HNO3(aq)+NO(g) How many grams of ammonia must you start with to make 800.00 L of a 0.150 M aqueous solution of nitric acid? Assume all the reactions give 100% yield.
The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in many modern chemical processes. In the first step of the Ostwald process, ammonia is reacted with oxygen gas to produce nitric oxide and water. What is the maximum mass of H2O that can be produced by combining 58.5 g of each reactant? 4NH3(g)+5O2(g)⟶4NO(g)+6H2O(g) mass: g H2O
9. The first step in industrial nitric acid production is the catalyzed oxidation of ammonia. Without a catalyst, a different reaction predominates: 4NH3(g) +302(g) 2N2( ) + 6H 20(g) When 0.0260 mol gaseous NHs and 0.0240 mol gaseous O-, are placed in a 1.00 L container at a certain temperature, the Ns concentration at equilibrium is 2.80x 10 3 M. Calculate Keg for the reaction at this temperature. Submit Answer Tries 0/99
The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in many modern chemical processes. In the first step of the Ostwald process, ammonia is reacted with oxygen gas to produce nitric oxide and water What is the maximum mass of H,O that can be produced by combining 88.9 g of each reactant? 4 NO(g)6 H2O(g) 4 NH2 (g)5 02(g) 8 Н,О mass:
The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in many modern chemical processes In the first step of the Ostwald process, ammonia is reacted with oxygen gas to produce nitric oxide and water. What is the maximum mass of H, O that can be produced by combining 57.1 g of each reactant? 4 NH3(g) + 502(g) → 4NO(g) + 6H2O(g) mass: - mass: ho
The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in many modern chemical processes. In the first step of the Ostwald process, ammonia is reacted with oxygen gas to produce nitric oxide and water. What is the maximum mass of H₂O that can be produced by combining 73.3 g of each reactant? 4NH₃(g) +5O₂(g) → 4NO(g) + 6H₂O(g) mass: _______ g H₂O