Nitric acid is a key industrial chemical, largely used to make fertilizers and explosives. The first step in its synthesis is the oxidation of ammonia. In this reaction, gaseous ammonia reacts with dioxygen gas to produce nitrogen monoxide gas and water. Suppose a chemical engineer studying a new catalyst for the oxidation of ammonia reaction finds that 990. liters per second of dioxygen are consumed when the reaction is run at 271. °C and the dioxygen is supplied at 0.30 atm. Calculate the rate at which nitrogen monoxide is being produced. Give your answer in kilograms per second. Be sure your answer has the correct number of significant digits. do kg

Nitric acid is a key industrial chemical, largely used to make fertilizers and explosives. The first step in its synthesis is the oxidation of ammonia. In this reaction, gaseous ammonia reacts with dioxygen gas to produce nitrogen monoxide gas and water. Suppose a chemical engineer studying a new catalyst for the oxidation of ammonia reaction finds that 990. liters per second of dioxygen are consumed when the reaction is run at 271. °C and the dioxygen is supplied at 0.30 atm. Calculate the rate at which nitrogen monoxide is being produced. Give your answer in kilograms per second. Be sure your answer has the correct number of significant digits. do kg

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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In the Haber reaction, patented by German chemist Fritz Haber in 1908, dinitrogen gas combines with dihydrogen gas to produce gaseous ammonia. This reaction 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 796. liters per second of dinitrogen are consumed when the reaction is run at 196. °C and the dinitrogen is supplied at 0.69 atm. Calculate the rate at which ammonia is being produced. Give your answer in kilograms per second. Round your answer to 2 significant digits.
Nitric acid is a key industrial chemical, largely used to make fertilizers and explosives. The first step in its synthesis is the oxidation of ammonia. In this reaction, gaseous ammonia reacts with dioxygen gas to produce nitrogen monoxide gas and water. Suppose a chemical engineer studying a new catalyst for the oxidation of ammonia reaction finds that 602. liters per second of dioxygen are consumed when the reaction is run at 222.°C and the dioxygen is supplied at 0.83atm. Calculate the rate at which nitrogen monoxide is being produced. Give your answer in kilograms per second. Round your answer to 2 significant digits. =____kg/s
Nitric acid is a key industrial chemical, largely used to make fertilizers and explosives. The first step in its synthesis is the oxidation of ammonia. In this reaction, gaseous ammonia reacts with dioxygen gas to produce nitrogen monoxide gas and water. Suppose a chemical engineer studying a new catalyst for the oxidation of ammonia reaction finds that 985. liters per second of dioxygen are consumed when the reaction is run at 241. °C and the dioxygen is supplied at 0.29 atm. Calculate the rate at which nitrogen monoxide is being produced. Give your answer in kilograms per second. Be sure your answer has the correct number of significant digits.
Mar In the Haber reaction, patented by German chemist Fritz Haber in 1908, dinitrogen gas combines with dihydrogen gas to produce gaseous ammonia. This reaction 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 285. liters per second of dinitrogen are consumed when the reaction is run at 222. °C and the dinitrogen is supplied at 0.13 atm. Calculate the rate at which ammonia is being produced. Give your answer in kilograms per second. Be sure your answer has the correct number of significant digits. Check Save For Later Submit Assignment student-followme-color 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use I Privacy Center Accessibility EPIC 中Exe MacBook Pro esc F2 F3 ODO F4 88 F6 F8 F12 F5 $ & 23 一 de 3. 4. 9 6 { A lock C 己 B. N W alt ontrol option command command option
When limestone (solid CaCO,) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete- the lime absorbs CO₂ from the air and turns back into hard, durable limestone. Suppose some calcium carbonate is sealed into a limekiln of volume 500. L. and heated to 520.0 °C. When the amount of CaCO, has stopped changing, it is found that 3.84 kg have disappeared. Calculate the pressure equilibrium constant K, this experiment suggests for the equilibrium between CaCO, and CaO at 520.0 °C. Round your answer to 2 significant digits. Note for advanced students: it's possible there was some error in this experiment, and the value it suggests for K, does not match the accepted value.
In the Haber reaction, patented by German chemist Fritz Haber in 1908, dinitrogen gas combines with dihydrogen gas to produce gaseous ammonia. This reaction 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 715. liters per second of dinitrogen are consumed when the reaction is run at 153. °C and the dinitrogen is supplied at 0.18 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 S Continue dallall 80 x10 X 802 S ? JUN 27 © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | A O Submit Assi tv .
Consider a vessel with a moveable piston. The initial volume of this vessel is 15.0 L, and inside the vessel is x moles of N2(g) and x moles of H2(g). The total pressure in the vessel is 2.00 bar. The reaction between N₂ and H₂ is initiated, and NH3 forms. N2(g) + 3 H2(g) →→→ 2NH3(g) If this reaction goes to completion, what will be the final volume of the vessel if the total pressure remains at 2.00 bar? 5.0 L 10.0 L 15.0 L 20.0 L
In the Haber reaction, patented by German chemist Fritz Haber in 1908, dinitrogen gas combines with dihydrogen gas to produce gaseous ammonia. This reaction 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 122. liters per second of dinitrogen are consumed when the reaction is run at 179. °C and the dinitrogen is supplied at 0.59 atm. Calculate the rate at which ammonia is being produced. Give your answer in kilograms per second. Round your answer to 2 significant digits. 0 kg V 0 x10 X
In order to produce solid iron, it first must bc processed from its orc, Fe2O1, in a blast furnace. During operation, CO gas (flue gas) is introduced into the furnace at 1650 °C and a pressure of 250 kPa. In this process flue gas reduces iron to its elemental form in the following reaction: 41. Fe;O30) COg Fe+ COz At one point in this process 256.0 L of CO was used to reduce iron ore. Assuming a complete reaction, how many grams of solid iron can be produced. Balanced chemical equation: Mass of Fe (in grams)
The human body burns glucose (C6H12O6) for energy according to this chemical reaction: C6H12O6+6O2→ 6CO2+6H2O The products of the reaction are carbon dioxide CO2 and water H2O Interestingly, all of the carbon dioxide and much of the water exits the body through the lungs: on every breath, the average person exhales 500.mL of air, which is typically enriched to 4% CO2 and 5% water vapor by volume. In short, when a person loses weight by dieting, the weight that is lost actually departs his body as a gas, every time he exhales. Each kilogram of body fat lost requires exhaling about 2.9kg of carbon dioxide. Calculate how many breaths it takes an average person to "exhale" 0.50kg of fat. Round your answer to the nearest thousand. You'll need to know that the density of CO2 is 2.0 kg/m^3 .
Ancient Romans built often out of bricks and mortar. A key ingredient in their mortar was quicklime (calcium oxide), which they produced by roasting limestone (calcium carbonate). 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid calcium carbonate (CACO) into solid calcium oxide and gaseous carbon dioxide. 2. Suppose 43.0 L of carbon dioxide gas are produced by this reaction, at a temperature of 250.0 °C and pressure of exactly 1 atm. Calculate the mass of calcium carbonate that must have reacted. Round your answer to 3 significant digits. Explanation Check O 2021 McGraw-Hill Education. All Rights Reserved Terms of Use Privacy Access MacBook Air 4 F7 II F8 A F10 O F3 9 FR . F6 F5 4.
Most of the sulfur used in the United States is chemically synthesized from hydrogen sulfide gas recovered from natural gas wells. In the first step of this synthesis, called the Claus process, hydrogen sulfide gas is reacted with dioxygen gas to produce gaseous sulfur dioxide and water. Suppose a chemical engineer studying a new catalyst for the Claus reaction finds that 592. liters per second of dioxygen are consumed when the reaction is run at 195. °℃ and the dioxygen is supplied at 0.48 atm. Calculate the rate at which sulfur dioxide is being produced. Give your answer in kilograms per second. Be sure your answer has the correct number of significant digits.