Ethylene (CH2CH2) is the starting point for a wide array of industrial chemical syntheses. For example, worldwide about 8.0 × 10 10 kg of polyethylene aremade from ethylene each year, for use in everything from household plumbing to artificial joints. Natural sources of ethylene are entirely inadequate to meetworld demand, so ethane (CH3 CH3) from natural gas is "cracked" in refineries at high temperature in a kinetically complex reaction that produces ethylene gasand hydrogen gas.Suppose an engineer studying ethane cracking fills a 50.0 L reaction tank with 16.0 atm of ethane gas and raises the temperature to 450. °C. She believesK₁= 0.080 at this temperature.Calculate the percent by mass of ethylene the engineer expects to find in the equilibrium gas mixture. Round your answer to 2 significant digits.Note for advanced students: the engineer may be mistaken about the correct value of K, and the mass percent of ethylene you calculate may not be what sheactually observes.☐ %☐ x10☑

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Answered: Ethylene (CH2CH2) is the starting point…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter4: Energy And Chemical Reactions

Section: Chapter Questions

Problem 122QRT

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Ethylene (CH₂CH₂) is the starting point for a wide array of industrial chemical syntheses. For example, worldwide about 8.0 × 10¹0 kg of polyethylene are made from ethylene each year, for use in everything from household plumbing to artificial joints. Natural sources of ethylene are entirely inadequate to meet world demand, so ethane (CH3CH3) from natural gas is "cracked" in refineries at high temperature in a kinetically complex reaction that produces ethylene gas and hydrogen gas. Suppose an engineer studying ethane cracking fills a 80.0 L reaction tank with 14.0 atm of ethane gas and raises the temperature to 850. °C. He believes K₂=0.60 at this temperature. alo Calculate the percent by mass of ethylene the engineer expects to find in the equilibrium gas mixture. Round your answer to 2 significant digits. Ar Note for advanced students: the engineer may be mistaken about the correct value of K, and the mass percent of ethylene you calculate may not be what he actually observes. % 0x₁…
Ethylene (CH₂CH₂) is the starting point for a wide array of industrial chemical syntheses. For example, worldwide about 8.0 × 10¹0 kg of polyethylene are made from ethylene each year, for use in everything from household plumbing to artificial joints. Natural sources of ethylene are entirely inadequate to meet world demand, so ethane (CH₂CH3) from natural gas is "cracked" in refineries at high temperature in a kinetically complex reaction that produces ethylene gas and hydrogen gas. Suppose an engineer studying ethane cracking fills a 35.0 L reaction tank with 35.0 atm of ethane gas and raises the temperature to 400. °C. He believes K₂=0.20 at this temperature. Calculate the percent by mass of ethylene the engineer expects to find in the equilibrium gas mixture. Round your answer to 2 significant digits. Note for advanced students: the engineer may be mistaken about the correct value of Kp and the mass percent of ethylene you calculate may not be what he actually observes.
Ethylene (CH2CH2) is the starting point for a wide array of industrial chemical syntheses. For example, worldwide about 8.0x10^10 kg of polyethylene are made from ethylene each year, for use in everything from household plumbing to artificial joints. Natural sources of ethylene are entirely inadequate to meet world demand, so ethane (CH3CH3) from natural gas is "cracked" in refineries at high temperature in a kinetically complex reaction that produces ethylene gas and hydrogen gas. Suppose an engineer studying ethane cracking fills a 75.0 L reaction tank with 23.0 atm of ethane gas and raises the temperature to 750.°C. He believes Kp=6.0 at this temperature. Calculate the percent by mass of ethylene the engineer expects to find in the equilibrium gas mixture. Round your answer to 2 significant digits.
12
The most extensively used organic compound in the chemical industry is ethene (C,H4). The two equations C2H4(g) + Cl2 (g) 2CH¾C1½(g) C2H4CI2 (g)=C2H;Cl(g) + HCl(g) represent the way in which vinyl chloride (C,H;CI) is syn- thesized for eventual use in polymeric plastics (polyvinyl chloride, PVC). The byproduct of the reaction, HCI, is now most cheaply made by this and similar reactions, rathcr than by dircct combination of H, and Cl2. Hcat is given off in the first reaction and taken up in the second. Describe how you would design an industrial process to maximize the yield of vinyl chloride.
Paylben
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Approximately 12 billion kilograms of phosphoric acid (H3PO4) are produced annually for fertilizers, detergents, and agents for water treatment. Phosphoric acid can be prepared by heating the mineral fluoroapatite (Ca5(PO4)3F) with sulphuric acid in the presence of water. Ca5(PO4)3F + 5H2SO4 + 10H20 → 3H3PO4 + 5CaSO4 2H20 + HF If every kilogram of fluoroapatite yields 390 g of phosphoric acid, what is the percent yield? percent
The U.S. proven natural gas reserves in 2013 were 323 trillion ft3 . How long will these reserves last if there are no imports or exports and if the U.S. annual rate of use of 24.5 trillion ft3 continues?
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At 1.00 atm and 0 °C, a 5.04 L mixture of methane (CH4) and propane (C₂H₂) was burned, producing 16.5 g CO₂. What was the mole fraction of each gas in the mixture? Assume complete combustion. Xmethane = Xpropane

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