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 1.5 L flask with 2.3 atm of ethylene gas and 5.0 atm of water vapor. When the mixture has come to equilibrium he determines that it contains 1.57 atm of ethylene gas and 4.27 atm of water vapor. The engineer then adds another 1.3 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.

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 1.5 L flask with 2.3 atm of ethylene gas and 5.0 atm of water vapor. When the mixture has come to equilibrium he determines that it contains 1.57 atm of ethylene gas and 4.27 atm of water vapor. The engineer then adds another 1.3 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.

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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olo 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 3.8 atm of ethylene gas and 1.5 atm of water vapor. When the mixture has come to equilibrium he determines that it contains 2.96 atm of ethylene gas and 0.66 atm of water vapor. The engineer then adds another 0.95 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. atm
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Hydrogen can be extracted from natural gas according to the following reaction: CH4(g) + CO2(g) = 2CO(g) + 2H₂(g) Kp = 4.5x103 at 825 K An 85.0L reaction container initially contains 22.3 kg of CH4 and 55.4 kg of CO2 at 825 K. Assuming ideal gas behavior, calculate the mass of H₂ (in grams) present in the reaction mixture at equilibrium...
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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
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 2.0 L flask with 1.6 atm of nitrogen dioxide gas. When the mixture has come to equilibrium she determines that it contains 1.1 atm of nitrogen dioxide gas. The engineer then adds another 0.80 atm of nitrogen dioxide, and allows the mixture to come to equilibrium again. Calculate the pressure of dinitrogen tetroxide after equilibrium is reached the second time. Round your answer to 2 significant digits.