While ethanol (CH3CH₂OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH₂CH₂) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 25 L tank with 12. mol of ethylene gas and 8.4 mol of water vapor. When the mixture has come to equilibriun he determines that it contains 6.1 mol of ethylene gas and 2.5 mol of water vapor. The engineer then adds another 3.0 mol of ethylene, and allows the mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. mol X 5 ? e

While ethanol (CH3CH₂OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH₂CH₂) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 25 L tank with 12. mol of ethylene gas and 8.4 mol of water vapor. When the mixture has come to equilibriun he determines that it contains 6.1 mol of ethylene gas and 2.5 mol of water vapor. The engineer then adds another 3.0 mol of ethylene, and allows the mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. mol X 5 ? e

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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Consider the equilibrium system described by the chemical reaction below. At equilibrium, a sample of gas from the system is collected into a 5.00 L flask at 1200 K. The flask is found to contain 2.81 g of CH, 1.25 g of CO, 15.1 g of cO, and 25.3 g of H, What is the value of Kc for this reaction? CH.(g) + CO,(9) = 2 CO(g) + 2 H,(g)
Iron and water react to form iron(III) oxide and hydrogen, like this: 2 Fe(s)+3 H,0(g)→ Fe,O3(s)+3 H,(g) At a certain temperature, a chemist finds that a 9.2 L reaction vessel containing a mixture of iron, water, iron(III) oxide, and hydrogen at equilibrium has the following composition: compound amount ol. Fe 4.85 g Ar H,O 1.44 g Fe,O3 2.98 g H2 2.51 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = 0 Ox10 Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility
While ethanol (CH,CH,OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH,CH,) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 100 L tank with 8.3 mol of ethylene gas and 32. mol of water vapor. When the mixture has come to equilibrium she determines that it contains 2.4 mol of ethylene gas and 26.1 mol of water vapor. The engineer then adds another 16. mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. || mol
A closed 1.00 L system initially containing 0.00200 mol H₂ and 0.00500 mol 1₂ at a given temperature is allowed to reach equilibrium Analysis of the equilibrium mixture shows that the amount of HI present at equilibrium is 0.00371 mol. Calculate the Kc at this temperature for the reaction. State whether the equilibrium is product-favored or reactant- favored at this temperature. H₂(g) +1₂(g) 2H1(g) Kc 31: The equilibrium is product-favored. Kc 31: The equilibrium is reactant-favored. Kc 0.032; The equilibrium is reactant-favored. Kc - 0.032; The equilibrium is product-favored.
"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 1.5L flask with 2.9 atm of carbon monoxide gas and 2.9 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 1.4 atm of carbon monoxide gas, 1.4 atm of water vapor and 1.5 atm of carbon dioxide. The engineer then adds another 0.97 atm of carbon monoxide, and allows the mixture to come to equilibrium again. Calculate the pressure of hydrogen after equilibrium is reached the second time. Round your answer to 2 significant digits. atm x10 Submit Assignment Continue 2021 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibility MacBook Air DII 888 F10 F8 F9 esc F6 F7 F4 F5 F3 F2 %23 $4 % - & 4. 5 8.
While ethanol (CH,CH,OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH,CH,) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 100 L tank with 45. mol of ethylene gas and 35. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 34. mol of ethylene gas and 24. mol of water vapor. The engineer then adds another 18. mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. | mol
4. Sulfuric acid is an important industrial chemical that is usually produced by a series of reactions. One of these involves an equilibrium between gaseous sulfur dioxide, oxygen, and sulfur trioxide. 2 SO,(g) + 0,(g) So,(g) If 2.5 mol of sulfur dioxide gas and 2.0 mol of oxygen gas are placed in a sealed 1.0 L container and allowed to reach equilibrium, 0.75 mol of sulfur dioxide remains. Use an ICE table to determine the concentration of the other gases at equilibrium. m
While ethanol (CH,CH,OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH,CH,) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 200. mL flask with 1.7 atm of ethylene gas and 2.2 atm of water vapor. When the mixture has come to equilibrium he determines that it contains 0.92 atm of ethylene gas and 1.42 atm of water vapor. olo Ar The engineer then adds another 1.1 atm Of water, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. atm
While ethanol (CH3CH2OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH2CH2) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 1.5 L flask with 4.8 atm of ethylene gas and 3.9 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 3.1 atm of ethylene gas and 2.2 atm of water vapor. The engineer then adds another 1.2 atm of ethylene, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. at atm 5
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While ethanol (CH, CH₂OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH₂CH₂) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 2.0 L flask with 2.1 atm of ethylene gas and 3.2 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 0.50 atm of ethylene gas and 1.6 atm of water vapor. The engineer then adds another 1.1 atm of water, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits.
Nitrogen dioxide is one of the many oxides of nitrogen (often collectively called "NOx") that are of interest to atmospheric chemistry. It can react with itself to form another form of NOx, dinitrogen tetroxide. A chemical engineer studying this reaction fills a 125.L tank at 13.°C with 16.mol of nitrogen dioxide gas. He then raises the temperature considerably, and when the mixture has come to equilibrium determines that it contains 6.9mol of nitrogen dioxide gas. The engineer then adds another 8.0mol of nitrogen dioxide, and allows the mixture to come to equilibrium again. Calculate the moles of dinitrogen tetroxide after equilibrium is reached the second time. Round your answer to 2 significant digits.