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2. The Ostwald process for the commercial production of nitric acid involves three steps: 4 NH3(g)...
The Ostwald process for the commercial production of nitric acid from ammonia and oxygen involves the steps in the table below. (a) Use the values of AHfº in Appendix 4 to calculate the value of AHO for each of the following reactions. Reaction AH 4 NH3(g) + 5 02(9) ► 4 NO(g) + 6 H20(9) 2 NO(g) + O2(g) +2 NO2(9) 3 NO2(g) + H20(1) - 2 HNO3(aq) + NO(g) (b) Write the overall equation for the production of nitric...
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 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 H2O that can be produced by combining 58.5 g of each reactant? 4NH3(g)+5O2(g)⟶4NO(g)+6H2O(g) mass: g H2O
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 2 O that can be produced by combining 63.1 g of each reactant? 4 NH 3 ( g ) + 5 O 2 ( g ) ⟶ 4 NO ( g ) +...
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
The first step in the Ostwald process for producing nitric acid is 4NH₃(g) +5O₂(g) → 4NO(g) + 6H₂O(g). If the reaction of 0.15kg of ammonia with 0.15kg of oxygen gas yields 87g of nitric oxide, what is the percent yield of this reaction?
The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (O2) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here: ?NH3(g)+?O2(g)→?NO(g)+?H2O(g) Part A What volume of O2 at 684 mmHg and 41 ∘C is required to synthesize 19.0 mol of NO? Express your answer to three significant figures and include the appropriate units. volume of O^2=
The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (O2) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here: ?NH3(g)+?O2(g)→?NO(g)+?H2O(g) What volume of O2 at 798 mmHg and 41 ∘C is required to synthesize 12.5 mol of NO? Express your answer to three significant figures and include the appropriate units.
The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (O2) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here: ?NH3(g)+?O2(g)→?NO(g)+?H2O(g) What volume of O2 at 912 mmHg and 41 ∘C∘C is required to synthesize 24.5 mol of NO? 750 mmHg = 1 bar R = 0.08314 L bar mol-1 K-1 Express your answer numerically in litres.