Answer is in images
Question 63 The Haber process is the synthesis of ammonia gas from hydrogen and nitrogen on...
QUESTION 24 The Born-Haber process is used to manufacture ammonia (NH3) from nitrogen gas and hydrogen gas at STP according to the following reaction: 3 H2(g) + N2(g) → 2 NH3(g) a. What is the volume of ammonia in the reaction vesselif 2.253 moles are produced? b. How many liters of nitrogen are needed to react with 50.2 g of hydrogen?
In the Haber–Bosch process, ammonia is synthesized from hydrogen and nitrogen gas. The equilibrium concentrations of NH3, H2, and N2 are 0.0040 M, 0.20 M, and 0.080 M, respectively. Determine the directional shift of the reaction for each of the following situations: i. All three concentrations are 0.20 M ii. All three concentrations are 2.0 M
Ammonia is created in the Haber process in a rigid container (nitrogen gas plus hydrogen gas react to form ammonia gas). 2 moles of hydrogen gas are mixed with 4 moles of nitrogen gas. The initial pressure exerted on the container is 5 atm. Assuming the reaction runs to completion, what will the pressure (in atm) on the vessel be after the reaction takes place?
The Haber-Bosch process is used to make ammonia from nitrogen and hydrogen: N2(g) + 3 H2(g) 2 NH3(g). A 10.0 L reactor at 450 °C is filled with 3 moles of nitrogen and 12 moles of hydrogen, K is 0.16 under these conditions.
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 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 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-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 converts atmospheric nitrogen to ammonia via reaction with hydrogen using a catalyst under high temperature and pressure. 2 kmol of N2 gas react with 4 kmol of H2 gas to create ammonia. Assume all of the limiting reagent is used up. (total 12 marks) a. Draw and label everything (as you go) (4 marks) b. Using the Extent of Reaction, identify the exit stream contents. (4 marks) c. Given that I have the same feeds above, but...
1. The cartoon below represents the reaction of nitrogen gas (N2) with hydrogen gas (H2) to synthesize ammonia (NHs). Industrially, this che pro mical process is called the Haber-Bosch cess, and is still a very important reaction in the manufacture of fertilizers. The ability to fix every day). It has been estimated that use of nitrogen-based fertilizers has doubled the world's a. The cartoon below shows 6 molecules of hydrogen gas and 2 molecules of nitrogen nitrogen and manufacture fertilizers...