In the Haber reaction, patented by German chemist Fritz Haber in 1908, dinitrogen gas combines with dihydrogen gas to produce gaseous ammonia. Thisreaction is now the first step taken to make most of the world's fertilizer.Suppose a chemical engineer studying a new catalyst for the Haber reaction finds that 101. liters per second of dinitrogen are consumed when the reaction isrun at 262. °C and the dinitrogen is supplied at 0.16 atm. Calculate the rate at which ammonia is being produced. Give your answer in kilograms per second.Round your answer to 2 significant digits.kg?

Given: The volume (V) of the dinitrogen gas (N2) is 101 L The pressure (P) of the dinitrogen gas…

Answered: In the Haber reaction, patented by…

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter5: Gases

Section: Chapter Questions

Problem 74E: Urea (H2NCONH2) is used extensively as a nitrogen source in fertilizers. It is produced commercially...

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Liquid oxygen was first prepared by heating potassium chlorate, KClO3, in a closed vessel to obtain oxygen at high pressure. The oxygen was cooled until it liquefied. 2KClO3(s)2KCl(s)+3O2(g) If 171 g of potassium chlorate reacts in a 2.70-L vessel, which was initially evacuated, what pressure of oxygen will be attained when the temperature is finally cooled to 25C? Use the preceding chemical equation and ignore the volume of solid product.
A four-liter tank is filled with propane gas, C3H8. The mass of the tank filled with gas is 1236 g. The pressure in the tank is 2.68 atm. The temperature in the room is 37C. The propane in the tank is used up under the same conditions of temperature and pressure. What is the mass of the empty tank?
Raoul Pictet, the Swiss physicist who first liquefied oxygen, attempted to liquefy hydrogen. He heated potassium formate, KCHO2, with KOH in a closed 2.50-Lvessel. KCHO2(s)+KOH(s)K2CO3(s)+H2(g) If 75.0 g of potassium formate reacts in a 2.50-L vessel, which was initially evacuated, what pressure of hydrogen will be attained when the temperature is finally cooled to 25C? Use the preceding chemical equation and ignore the volume of solid product.
94 Mining engineers often have to deal with gases when planning for the excavation of coal. Some of these gases, including methane, can be captured and used as fuel to support the mining operation. For a particular mine, 2.4 g of CH4 is present for every 100.0 g of coal that is extracted. If 45.6% of the methane can be captured and the daily production of the mine is 580 metric tons of coal, how many moles of methane could be obtained per day?
97 Homes in rural areas where natural gas service is not available often rely on propane to fuel kitchen ranges. The propane is stored as a liquid, and the gas to be burned is produced as the liquid evaporates. Suppose an architect has hired you to consult on the choice of a propane tank for such a new home. The propane gas consumed in 1.0 hour by a typical range burner at high power would occupy roughly 165 L at 25°C and 1.0 atm, and the range chosen by the client will have six burners. If the tank under consideration holds 500.0 gallons of liquid propane, what is the minimum number of hours it would take for the range to consume an entire tankful of propane? The density of liquid propane is 0.5077 kg/L.
105 The decomposition of mercury(II) thiocyanate produces an odd brown snake-like mass that is so unusual the process was once used in fireworks displays. There are actually several reactions that take place when the solid Hg(SCN)2 is ignited: 2Hg(SCN)2(s)2HgS(s)+CS2(s)+C3N4(s)CS2(s)+3O2(g)CO2(g)+2SO2(g)2C3N4(s)3(CN)2(g)+N2(g)HgS(s)+O2(g)Hg(l)+SO2(g) A 42.4-g sample of Hg(SCN)2 is placed into a 2.4-L vessel at 21°C. The vessel also contains air at a pressure of 758 torr. The container is sealed and the mixture is ignited, causing the reaction sequence above to occur. Once the reaction is complete, the container is cooled back to the original temperature of 21°C. (a) Without doing numerical calculations, predict whether the final pressure in the vessel will be greater than, less than, or equal to the initial pressure. Explain your answer. (b) Calculate the final pressure and compare your result with your prediction. (Assume that the mole fraction of O2 in air is 0.21.)
Butane, C4H10, is an easily liquefied gaseous fuel. Calculate the density of butane gas at 0.857 atm and 22C. Give the answer in grams per liter
You have a gas, one of the three known phosphorus-fluorine compounds (PF3, PF3, and P2F4). To find out which, you have decided to measure its molar mass. (a) First, yon determine that the density of the gas is 5.60 g/L at a pressure of 0.971 atm and a temperature of 18.2 C. Calculate the molar mass and identify the compound. (b) To check the results from part (a), you decide to measure the molar mass based on the relative rales of effusion of the unknown gas and CO2. You find that CO2 effuses at a rate of 0.050 mol/min, whereas the unknown phosphorus fluoride effuses at a rate of 0.028 mol/min. Calculate the molar mass of the unknown gas based on these results.

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