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

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

"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 3.1 atm of carbon monoxide gas and 3.6 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 1.0 atm of carbon monoxide gas, 1.5 atm of water vapor and 2.1 atm of carbon dioxide. The engineer then adds another 0.90 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 C [