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 125 L tank with 52. mol of ethylene gas and 51. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 33. mol of ethylene gas and 32. mol of water vapor. The engineer then adds another 17. 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 125 L tank with 52. mol of ethylene gas and 51. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 33. mol of ethylene gas and 32. mol of water vapor. The engineer then adds another 17. 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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Suppose a 250. mL flask is filled with 1.0 mol of N, and 2.0 mol of NH,. This reaction becomes possible: N2 (g) + 3H,(g) – 2NH, (g) 2NH3 (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 H, NH, initial ? change equilibrium
Steam reforming of methane (CH4) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many important industrial chemical syntheses. An industrial chemist studying this reaction fills a 25.0 L tank with 8.8 mol of methane gas and 2.8 mol of water vapor, and when the mixture has come to equilibrium measures the amount of carbon monoxide gas to be 2.0 mol. Calculate the concentration equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to 2 significant digits. K = 0 x10 X
1.00 g each of CO, H2O, and H2ar4e sealed in a 1.41 L vessel and brought to equilibrium. How many grams of CO2will be present at equilibrium? CO + H2O <--> CO2+ H2 Kc = 23.2 (all gases)
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 31. mol of nitrogen dioxide gas. When the mixture has come to equilibrium he determines that it contains 12. mol of nitrogen dioxide gas. The engineer then adds another 10. 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 Х G
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 75 L tank with 5.6 mol of ethylene gas and 7.7 mol of water vapor. When the mixture has come to equilibrium he determines that it contains 2.3 mol of ethylene gas and 4.4 mol of water vapor. The engineer then adds another 2.8 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 x10
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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
At a certain temperature, 0.365 mol of CH4 and 0.736 mol of H2O is placed in a 4.00 L container. CH4+2H2O<------->CO2+4H2 At equilibrium, 5.68 g of CO2 is present. Calculate Kc.
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"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 25 L tank with 11. mol of carbon monoxide gas and 12. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 6.9 mol of carbon monoxide gas, 7.9 mol of water vapor and 4.1 mol of hydrogen gas. The engineer then adds another 3.0 mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of carbon dioxide after equilibrium is reached the second time. Round your answer to 2 significant digits. mol