Calculating the reaction rate of one reactant from that of anotherNitric acid is a key industrial chemical, largely used to make fertilizers and explosives. The first step in its synthesis is the oxidation ofammonia. 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 687. liters per second of dioxygen areconsumed when the reaction is run at 158. °C and the dioxygen is supplied at 0.90 atm. Calculate the rate at which nitrogen monoxide isbeing produced. Give your answer in kilograms per second. Round your answer to 2 significant digits.kgSx10☑كUndo

Answered: Calculating the reaction rate of one…

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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Iron reacts with oxygen gas to form a mixture of FeO and Fe₂O₃ when the supply of oxygen is regulated. A sample of 20.00 g iron metal reacts with oxygen gas to form 28.10 g iron oxide mixture, and all of the iron metal was consumed. What is the mass in g of FeO that were produced in the mixture?
Acetylene torches are used for welding. These torches use a mixture of acetylene gas, C2H2C2H2, and oxygen gas, O2O2 to produce the following combustion reaction: 2C2H2(g)+5O2(g)→4CO2(g)+2H2O(g)2C2H2(g)+5O2(g)→4CO2(g)+2H2O(g) Part A Imagine that you have a 7.00 LL gas tank and a 4.50 LL gas tank. You need to fill one tank with oxygen and the other with acetylene to use in conjunction with your welding torch. If you fill the larger tank with oxygen to a pressure of 125 atmatm , to what pressure should you fill the acetylene tank to ensure that you run out of each gas at the same time? Assume ideal behavior for all gases. Express your answer with the appropriate units.
One commercial system removes SO2 emissions from smoke at 95.0°C by the following set of balanced reactions: SO2(g) + Cl2 → SO2Cl2(g) SO2Cl2 + 2H2O → H2SO4 + 2HCl H2SO4 + Ca(OH)2 → CaSO4(s) + 2H2O Assuming the process is 0.86 % efficient, how many grams of CaSO4 may be produced from 91 g of SO2? Report your answer to 3 sig figs.
Adding helium to a balloon increased its volume from 479.9 mL to 2.961 L. If the final number of moles of helium in the balloon is 16.0 mol, what was the initial number of moles of helium in the balloon? Assume the balloon contained only helium initially. n = mol
Pennies that are currently being minted are composed of zinc coated with copper. A student determines the mass of a penny to be 2.482 g and then makes several scratches in the copper coating (to expose the underlying zinc). The student puts the scratched penny in hydrochloric acid, where the following reaction occurs between the zinc and the HCl (the copper remains undissolved): Zn(s) + 2 HCl(aq) --------> H2(g) + ZnCl2(aq)The student collects the hydrogen produced over water at 25°C. The collected gas occupies a volume of 0.899 L at a total pressure of 791 mmHg. Calculate the percent zinc (by mass) in the penny. (Assume that all the Zn in the penny dissolves.)
What is the easiest process to get to the result?
27 A chemist prepares a solution of sodium chloride (NaCl) by measuring out 0.50 g of NaCl into a 250. mL volumetric flask and filling to the mark with distilled water. Calculate the molarity of Cl anions in the chemist's solution. do Be sure your answer is rounded to 2 significant digits. 18 Ar mol x10 L Submit Assignment Continue 2022 McGraw Hill LLC. AIl Rights Reserved. Terms of Use Privacy Center Accessibility Show All IMG-6095.jpg IMG-6096.jpg IMG-6097.jpg IMG-6098.jpg IMG-6099.jpg MacBook Air DD DII F12 F11 F10 F9 80 F7 F8 F6 F5 F4 esc F2 F3 F1 & % @ # 7 8 3 4 5 6 1 2 { P E R Y Q W %24
62. Antacid Fizz When an antacid tablet dissolves in water, the fizz is due to a reaction between sodium hydrogen carbonate (NaHCO3), also called sodium bicarbonate, and citric acid (H₂CH₂O₂). 3NaHCO3(aq) + H₂CH₂O,(aq) → 3CO₂(g) + 3H₂O(l) + Na, C₂H₂O₂(aq) How many moles of Na₂C,H,O, can be produced if one tablet containing 0.0119 mol of NaHCO is dissolved?
Q11 Kindly solve this question in 20 minutes and get the thumbs up Please show me neat and clean work for it By hand solution needed
A reaction generates hydrogen gas, H2, as a product. The reactants are mixed and sealed in a 250-mL vessel. After 20.0 minutes, 3.91x10-2 mol H2 have been generated. Calculate the final concentration (in M) of H2 gas.
Acetylene torches are used for welding. These torches use a mixture of acetylene gas, C₂ H₂, and oxygen gas, O₂ to produce the following combustion reaction: 2C₂ H2(g) + 5O2 (g)→4CO2 (g) + 2H₂O(g) Part A Imagine that you have a 7.00 L gas tank and a 2.00 L gas tank. You need to fill one tank with oxygen and the other with acetylene to use in conjunction with your welding torch. If you fill the larger tank with oxygen to a pressure of 135 atm, to what pressure should you fill the acetylene tank to ensure that you run out of each gas at the same time? Assume ideal behavior for all gases. Express your answer with the appropriate units. ► View Available Hint(s) P = 48.4 Submit Previous Answers atm 巴」? X Incorrect; Try Again; 4 attempts remaining
The extraction of aluminum metal from the aluminum hydroxide found in bauxite by the Hall-Héroult process is one of the most remarkable success stories of 19th century chemistry, turning aluminum from a rare and precious metal into the cheap commodity it is today. In the first step, aluminum hydroxide reacts to form alumina Al2O3 and water: 2Al(OH)3(s) + Al2O3(s) -> 3H2O(g) In the second step, alumina Al2O3 and carbon react to form aluminum and carbon dioxide: 2Al2O3(s) + 3C(s) + 4Al(s) -> 3CO2(g) Suppose the yield of the first step is 74.% and the yield of the second step is 76.% . Calculate the mass of aluminum hydroxide required to make 4.0kg of aluminum. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.

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