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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 50 L tank with 6.5 mol of nitrogen dioxide gas. When the mixture has come to equilibrium he determines that it contains 4.8 mol of nitrogen dioxide gas. The engineer then adds another 3.3 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 X Ś ?

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 6.5 mol of nitrogen dioxide gas. When the mixture has come to equilibrium he determines that it contains 4.8 mol of nitrogen dioxide gas. The engineer then adds another 3.3 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 X Ś ?

World of Chemistry, 3rd edition
World of Chemistry, 3rd edition
3rd Edition
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Chapter17: Equilibrium
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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 50 L tank with 6.5 mol of nitrogen dioxide gas. When the mixture has come to equilibrium he determines that it contains 4.8 mol of nitrogen dioxide gas. The engineer then adds another 3.3 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. 00. Ar mol x10 Ś ? Explanation © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility Check 0:
Transcribed Image Text: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 6.5 mol of nitrogen dioxide gas. When the mixture has come to equilibrium he determines that it contains 4.8 mol of nitrogen dioxide gas. The engineer then adds another 3.3 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. 00. Ar mol x10 Ś ? Explanation © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility Check 0:
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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 75 L tank with 32. mol of ethylene gas and 28. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 25.4 mol of ethylene gas and 21.4 mol of water vapor. The engineer then adds another 9.3 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. olo Ar mol x10 X Ś ? Explanation © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility Check
Transcribed Image Text: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 75 L tank with 32. mol of ethylene gas and 28. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 25.4 mol of ethylene gas and 21.4 mol of water vapor. The engineer then adds another 9.3 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. olo Ar mol x10 X Ś ? Explanation © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility Check
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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 2.0 L flask with 2.5 atm of carbon monoxide gas and 2.6 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 1.3 atm of carbon monoxide gas, 1.4 atm of water vapor and 1.2 atm of carbon dioxide. The engineer then adds another 0.63 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. 0 atm x10 X 3 ? Explanation © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility Check 0: A olo Ar 1
Transcribed Image Text:"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 2.0 L flask with 2.5 atm of carbon monoxide gas and 2.6 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 1.3 atm of carbon monoxide gas, 1.4 atm of water vapor and 1.2 atm of carbon dioxide. The engineer then adds another 0.63 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. 0 atm x10 X 3 ? Explanation © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility Check 0: A olo Ar 1
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