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 1.9 mol of ethylene gas and 5.7 mol of water vapor. When the mixture has come to equilibrium he determines that it contains 0.97 mol of ethylene gas and 4.77 mol of water vapor. The engineer then adds another 0.95 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

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 1.9 mol of ethylene gas and 5.7 mol of water vapor. When the mixture has come to equilibrium he determines that it contains 0.97 mol of ethylene gas and 4.77 mol of water vapor. The engineer then adds another 0.95 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

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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A mixture of water and graphite is heated to 890 K in a 14.5-L container. When the system comes to equilibrium it contains 0.835 mol each of CO gas and H2 gas and 0.182 mol of H2O gas and some graphite. Some O2 gas is added to the system and a spark is applied so that the H2 reacts completely with the O2, forming H2O. Find the amount of CO in the flask when the system returns to equilibrium.
A sample of N₂H6CO₂ weighing 22.5 grams is heated to 80°C in a 1.0 L container. All of the salt sublimes into NH3(g) and CO₂(g) according to the following equilibrium process. N₂H6CO₂ (s) + CO₂ (g) + 2NH3 (g) Determine the partial pressure of the NH3(g) in the system in atmospheres. This discussion is closed. M CAL -:00- 0:50- CI 2:00 Submit Answer Tries 0/99 3 F1 @ 2 ост 21 9: F2 3 80 F3 $ 4 10 a F4 % 5 S F5 6 tv A MacBook Air C F6 & 7 F7 ( Î DII FB F9 F10 F11 54 F13 Send 22
A sample of NH4HS(s) is placed into a 1.60 L vessel containing 0.170 g NH3. What is the total gas pressure when the system reaches equilibrium at 298.15 K? The reaction is: NH4HS(s) = NH3(g) + H2S(g) Kp = 0.108
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...
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:
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
"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 5.0 L flask with 1.0 atm of carbon monoxide gas and 2.5 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 0.69 atm of carbon monoxide gas, 2.19 atm of water vapor and 0.31 atm of hydrogen gas. The engineer then adds another 0.25 atm of carbon monoxide, and allows the mixture to come to equilibrium again. Calculate the pressure of carbon dioxide after equilibrium is reached the second time. Round your answer to 2 significant digits. atm
Phosphorus pentachloride decomposes according to the chemical equation PCl5(g)↽−−⇀PCl3(g)+Cl2(g)?c=1.80 at 250 ∘C A 0.3388 mol sample of PCl5(g) is injected into an empty 4.40 L reaction vessel held at 250 ∘C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium. [PCl5]= ____________M [PCl3]= ____________M
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.
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
"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 500. mL flask with 0.82 atm of carbon monoxide gas and 0.85 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 0.33 atm of carbon monoxide gas, 0.36 atm of water vapor and 0.49 atm of hydrogen gas. The engineer then adds another 0.41 atm of carbon monoxide, and allows the mixture to come to equilibrium again. Calculate the pressure of carbon dioxide after equilibrium is reached the second time. Round your answer to 2 significant digits. atm
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