One way to prevent emission of the pollutant NO from industrial plants is by catalyzed reaction with NH3 according to the reaction: 4 NH3(g) + 4 NO(g) + O2(g) \rightarrow→ 4 N2(g) + 6 H2(g) If the reaction takes place at 750 Torr and 365oC how many grams of ammonia are needed to treat 1000 L of NO gas?
One way to prevent emission of the pollutant NO from industrial plants is by catalyzed reaction...
1. Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the equation: 3 H2(g) + N2(g) → 2 NH3(2) - How many grams of H2 are needed to produce 14.43 g of NH3? 2. When propane (C2H8) burns, it reacts with oxygen gas to produce carbon dioxide and water. The unbalanced equation for this reaction is... CzHz (g) + O2(g) → CO2(g) + H2O(g) This type of reaction is referred to as a complete...
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 Haber-Bosch process is a very important industrial process. In the Haber-Bosch process, hydrogen gas reacts with nitrogen gas to produce ammonia according to the equation 3H2(g)+N2(g)→2NH3(g)3H2(g)+N2(g)→2NH3(g) The ammonia produced in the Haber-Bosch process has a wide range of uses, from fertilizer to pharmaceuticals. However, the production of ammonia is difficult, resulting in lower yields than those predicted from the chemical equation. 1.36 g H2 is allowed to react with 9.75 g N2, producing 1.75 g NH3 What is the...
The Haber-Bosch process is a very important industrial process. In the Haber-Bosch process, hydrogen gas reacts with nitrogen gas to produce ammonia according to the equation 3H2(g)+N2(g)→2NH3(g) The ammonia produced in the Haber-Bosch process has a wide range of uses, from fertilizer to pharmaceuticals. However, the production of ammonia is difficult, resulting in lower yields than those predicted from the chemical equation. 1.43 g H2 is allowed to react with 9.70 g N2, producing 2.31 g NH3. Part A: What...
The Haber-Bosch process is a very important industrial process. In the Haber Process, hydrogen gas reacts with nitrogen gas to produce ammonia according to the equation 3H2(g) + N2(g) ---> 2NH3(g) The ammonia produced in the Haber process has a wide range of uses from fertilizer to pharmaceuticals. However, the production of ammonia is difficult, resulting in lower yields than those predicted from the chemical equation. 1.57 g H2 is allowed to react with 9.87 g N2, producing 1.69 g Nh3....
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 Haber-Bosch process is a very important industrial process. In the Haber-Bosch process, hydrogen gas reacts with nitrogen gas to produce ammonia according to the equation 3H2(g)+N2(g)→2NH3(g) The ammonia produced in the Haber-Bosch process has a wide range of uses, from fertilizer to pharmaceuticals. However, the production of ammonia is difficult, resulting in lower yields than those predicted from the chemical equation. 1.26 g H2 is allowed to react with 9.75 g N2, producing 1.63 g NH3. Part A) What...
The Haber-Bosch process is a very important industrial process. In the Haber-Bosch process, hydrogen gas reacts with nitrogen gas to produce ammonia according to the equation 3H2(g)+N2(g)→2NH3(g) The ammonia produced in the Haber-Bosch process has a wide range of uses, from fertilizer to pharmaceuticals. However, the production of ammonia is difficult, resulting in lower yields than those predicted from the chemical equation. 1.10 g H2 is allowed to react with 9.72 g N2, producing 1.68 g NH3. Part A What...
The Haber-Bosch process is a very important industrial process. In the Haber-Bosch process, hydrogen gas reacts with nitrogen gas to produce ammonia according to the equation 3H2(g)+N2(g)→2NH3(g) The ammonia produced in the Haber-Bosch process has a wide range of uses, from fertilizer to pharmaceuticals. However, the production of ammonia is difficult, resulting in lower yields than those predicted from the chemical equation. 1.94 g H2 is allowed to react with 10.1 g N2, producing 1.59 g NH3. Part A What...
1. Given the following reaction: C(s) + O2(g) → CO2(g) If 75 grams of carbon were to be combusted, what is the maximum amount of CO2 that could be generated? 2. Given the following reaction: N2(g) + 3 H2(g) → 2 NH3 (g) If 70 grams of nitrogen gas are consumed in the reaction, what is the maximum amount of ammonia gas that can be produced?