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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 (CH3 CH3) from natural gas is "cracked" in refineries at high temperature in a kinetically complex reaction that produces ethylene gas and hydrogen gas. 圖 Suppose an engineer studying ethane cracking fills a 50.0 L reaction tank with 20.0 atm of ethane gas and raises the temperature to 600. °C. She believes Kp = 0.70 at this temperature. dlo 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 Kp, and the mass percent of ethylene you calculate may not be what she actually observes. 99 % X 5 ? Explanation Check

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 (CH3 CH3) from natural gas is "cracked" in refineries at high temperature in a kinetically complex reaction that produces ethylene gas and hydrogen gas. 圖 Suppose an engineer studying ethane cracking fills a 50.0 L reaction tank with 20.0 atm of ethane gas and raises the temperature to 600. °C. She believes Kp = 0.70 at this temperature. dlo 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 Kp, and the mass percent of ethylene you calculate may not be what she actually observes. 99 % X 5 ? Explanation Check

Chemistry
Chemistry
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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
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Ethylene (CH₂CH₂) is the starting point for a wide array of industrial chemical syntheses. For example, worldwide about 8.0 × 100 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 50.0 L reaction tank with 20.0 atm of ethane gas and raises the temperature to 600. °C. She believes K = 0.70 at this temperature. р 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 she actually observes. % x10 X Ś ? Explanation © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility Check 81 KI
Transcribed Image Text:Ethylene (CH₂CH₂) is the starting point for a wide array of industrial chemical syntheses. For example, worldwide about 8.0 × 100 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 50.0 L reaction tank with 20.0 atm of ethane gas and raises the temperature to 600. °C. She believes K = 0.70 at this temperature. р 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 she actually observes. % x10 X Ś ? Explanation © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility Check 81 KI
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Sulfuric acid is essential to dozens of important industries from steelmaking to plastics and pharmaceuticals. More sulfuric acid is made than any other industrial chemical, and world production exceeds 2.0 × kg per year. 10¹1 The first step in the synthesis of sulfuric acid is usually burning solid sulfur to make sulfur dioxide gas. Suppose an engineer studying this reaction introduces 2.6 kg of solid sulfur and 6.50 atm of oxygen gas at 700. °C into an evacuated 60.0 L tank. The engineer believes K₂=0.38 for the reaction at this temperature. Calculate the mass of solid sulfur she expects to be consumed when the reaction reaches equilibrium. Round your answer to 2 significant digits. olo Note for advanced students: the engineer may be mistaken in her belief about the value of K, and the consumption of sulfur you calculate may not be what she actually observes. Ar kg x10 X Ś ? Explanation © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility Check A K
Transcribed Image Text:Sulfuric acid is essential to dozens of important industries from steelmaking to plastics and pharmaceuticals. More sulfuric acid is made than any other industrial chemical, and world production exceeds 2.0 × kg per year. 10¹1 The first step in the synthesis of sulfuric acid is usually burning solid sulfur to make sulfur dioxide gas. Suppose an engineer studying this reaction introduces 2.6 kg of solid sulfur and 6.50 atm of oxygen gas at 700. °C into an evacuated 60.0 L tank. The engineer believes K₂=0.38 for the reaction at this temperature. Calculate the mass of solid sulfur she expects to be consumed when the reaction reaches equilibrium. Round your answer to 2 significant digits. olo Note for advanced students: the engineer may be mistaken in her belief about the value of K, and the consumption of sulfur you calculate may not be what she actually observes. Ar kg x10 X Ś ? Explanation © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility Check A K
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This one is a little different, but can u answer it as well

Nitrogen forms a surprising number of compounds with oxygen. A number of these, often given the collective symbol NOx (for "nitrogen + x oxygens") are serious contributors to air pollution. They can often be interconverted, sometimes by reaction with oxygen or ozone (03) in the air. An atmospheric scientist decides to study the reaction between nitrogen trioxide and nitrogen monoxide that produces nitrogen dioxide. He fills a stainless steel reaction chamber with 1.5 atm of nitrogen trioxide gas and 8.3 atm of nitrogen monoxide gas and raises the temperature considerably. At equilibrium he measures the mole fraction of nitrogen dioxide to be 0.19. Calculate the pressure equilibrium constant K for the equilibrium between nitrogen trioxide, nitrogen monoxide, and nitrogen dioxide at the final temperature р of the mixture. olo Round your answer to 2 significant digits. Ar K₁ = 0x₁ P Ś ? Explanation © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility Check x10 X 0: A 1
Transcribed Image Text:Nitrogen forms a surprising number of compounds with oxygen. A number of these, often given the collective symbol NOx (for "nitrogen + x oxygens") are serious contributors to air pollution. They can often be interconverted, sometimes by reaction with oxygen or ozone (03) in the air. An atmospheric scientist decides to study the reaction between nitrogen trioxide and nitrogen monoxide that produces nitrogen dioxide. He fills a stainless steel reaction chamber with 1.5 atm of nitrogen trioxide gas and 8.3 atm of nitrogen monoxide gas and raises the temperature considerably. At equilibrium he measures the mole fraction of nitrogen dioxide to be 0.19. Calculate the pressure equilibrium constant K for the equilibrium between nitrogen trioxide, nitrogen monoxide, and nitrogen dioxide at the final temperature р of the mixture. olo Round your answer to 2 significant digits. Ar K₁ = 0x₁ P Ś ? Explanation © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility Check x10 X 0: A 1
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