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 30. mol of ethylene gas and 27. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 9.0 mol of ethylene gas and 6.0 mol of water vapor. The engineer then adds another 14. 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

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 30. mol of ethylene gas and 27. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 9.0 mol of ethylene gas and 6.0 mol of water vapor. The engineer then adds another 14. 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

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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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 75 L tank with 14, mol of nitrogen dioxide gas. When the mixture has come to equilibrium she determines that It contains 4.2 mol of nitrogen diaxide gas. The engineer then adds another 4.7 mel of nitrogen diaxide, 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.
Suppose à 250. mL flask is filled with 1.3 mol of CO, 1.8 mol of H,O and 1.6 mol of H,. This reaction becomes possible: co() +H,0(g) =CO,e)+H,(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of H,. You can leave out the M symbol for molarity. CO H,0 Co, H, initial change equilibrium Explanation Check © 2021 McGraw-Hill Education. All Rights Roserved Terms of Use Privacy 1 Ace O Type here to search
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 with 47. mol of nitrogen dioxide gas. When the mixture has come to equilibrium he determines that it contains 22. mol of nitrogen dioxide gas. The engineer then adds another 16. mol 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. ||mol x10
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 25.0 L tank with 6.9 mol of ethylene gas and 11. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 1.5 mol of ethylene gas and 5.6 mol of water vapor. The engineer then adds another 2.8 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. I mol Ox10
Suppose a 500. mL flask is filled with 0.30 mol of SO, and 1.2 mol of SO3. This reaction becomes possible: 2SO, (g) +O,(g) 2SO3 Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of O,. You can leave out the M symbol for molarity. so, SO2 O2 initial change equilibrium
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
Nitrogen dioxide and water react to form nitric acid and nitrogen monoxide, like this: 3 NO₂(9)+H₂O(1)→2 HNO3(aq) + NO(g) At a certain temperature, a chemist finds that a 4.4 L reaction vessel containing a mixture of nitrogen dioxide, water, nitric acid, and nitrogen monoxide at equilibrium has the following composition: compound amount NO₂ 10.6 g H₂O 138.4 g HNO3 21.8 g NO 19.6 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. с K = [] x10 ×
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
"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 200. mL flask with 2.3 atm of carbon monoxide gas and 4.0 atm of water vapor. When the mixture has come to equilibrium he determines that it contains 0.90 atm of carbon monoxide gas, 2.6 atm of water vapor and 1.4 atm of carbon dioxide. The engineer then adds another 1.0 atm of water, 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. 0 atm x10 X
A mixture of 0.100 mol of SO2 and 0.100 mol of O2 is placed in a reaction container and allowed to react until equilibrium is established. 2 SO2 (g) + O2 (g) -> 2 SO3 At equilibrium, 0.0916 mol of SO3 is present. a. What is the composition of the equilibrium mixture in terms of moles of each substance present? (Hint: Stoichiometry!) b. If the container size is 3.0 L, what is the value of the equilibrium constant?
Suppose a 500. mL flask is filled with 1.4 mol of N, and 1.3 mol of NO. This reaction becomes possible: N,(2) +0,(2)- -2NO(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of N,. You can leave out the M symbol for molarity. N2 O2 NO initial change equilibrium olo
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 50 L tank with 22. mol of nitrogen dioxide gas. When the mixture has come to equilibrium she determines that it contains 6.0 mol of nitrogen dioxide gas. The engineer then adds another 5.5 mol 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. mol D X S