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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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.
Ethanol, C₂H6O, is most often blended with gasoline - usually as a 10 percent mix - to create a fuel called gasohol. Ethanol is a renewable resource and ethanol-blended fuels, like gasohol, appear to burn more efficiently in combustion engines. The combustion of one mole of ethanol releases 326.7 kcal of energy. The combustion of one mole of 2-methylhexane, C7H16, releases 1.150 × 10³ kcal of energy. How much energy is released during the complete combustion of 450. grams of 2-methylhexane? kcal Assuming the same efficiency, would 450. grams of ethanol provide more, less, or the same amount of energy as 450. grams of 2- methylhexane?
For a particular isomer of Cg H₁g, the combustion reaction produces 5108.7 kJ of heat per mole of Cg H₁ (g) consumed, under standard conditions. C8H18 (g) + -25 0₂(g) →→→ 8 CO₂(g) + 9 H₂O(g) AH; = ΔΗ What is the standard enthalpy of formation of this isomer of Cg H₁8 (g)? 18 -208.5 Incorrect ▲Hixn = -5108.7 kJ/mol kJ/mol
A) Ethanol, C2H6O, is most often blended with gasoline - usually as a 10 percent mix - to create a fuel called gasohol. Ethanol is a renewable resource and ethanol-blended fuels, like gasohol, appear to burn more efficiently in combustion engines. The combustion of one mole of ethanol releases 326.7 kcal of energy.The combustion of one mole of 2-methylhexane, C7H16, releases 1.150×103 kcal of energy. How much energy is released during the complete combustion of 495 grams of 2-methylhexane ?------------- kcalAssuming the same efficiency, would 495 grams of ethanol provide more, less, or the same amount of energy as 495 grams of 2-methylhexane? --------- B) Combustion reactions are exothermic. The heat of reaction for the combustion of 2-methylheptane, C8H18, is 1.306×103 kcal/mol. What is the heat of combustion for 2-methylheptane in kcal/gram?--------- kcal/gramHow much heat will be given off if molar quantities of 2-methylheptane react according to the following equation? 2 C8H18+25…
(b) Study the following themochemical data very carefully: Ciz(g) - 2ci(g) I2(g) IC(g) - 1(g) + CI(g) I2(s) → 12(g) AH° = 242.3 kJ AH° = 151.0 kJ 21(g) AH° = 211.3 kJ AH° = 62.8 kJ I2(s) reacts with Cl2(g) to produce ICI(g). Write the chemical equation to produce ONLY one mole of ICI(g) (i) Calculate AH° for the reaction of I2(s) with Cl2(g) to form 1 mole of ICI(g). Use all the data given above. (ii) What law did you use to calculate AH° above? (iii) What are the names of the following processes? I2(s) → 12(g) I2(g) 21(g) ICI(g) I(g) + Cl(g)
Write a balanced chemical reaction for the incomplete combustion of propane, C3H8C3H8 in oxygen gas to form carbon monoxide gas as one of the products.
Write a balanced chemical equation for the reaction that occurswhen (a) titanium metal reacts with O2(g); (b) silver(I)oxide decomposes into silver metal and oxygen gas whenheated; (c) propanol, C3H7OH(l) burns in air; (d) methyltert-butyl ether, C5H12O(l), burns in air.
Based on the reactions: 2NO2 (g) + 2N0 (g) + O2 (g) – – > 2N½O4 (g) ; AH = -228.54 kJ 4NO (g) +2N2O (g) + 50, (5) – – > 4N,O4 (g) ; AH,=-488.46 kJ 2NO (g) + O2 (g) – - > N,O4 (g) ; AH3 = –171.34 kJ- Use Hess's Law to calculate AH for: 4N204 (g) - - > 2N½O (g) + 302 (9) + 4NO2 (g)
The FDA-recommended daily allowance for fat in a 2,000 calorie diet is 77g. A. What is the max number of Calories which come from fat while still following this guideline? What is the total percent of daily allowance that can come from fat? The Atwater System provides a generalized value of 9.1 Cal/g of fat. B. Write the chemical equation and calculate the enthalpy of the combustion of stearin( C57H11006). 1 cal = 4184 Joules
Ethanol, C2H6O, is most often blended with gasoline - usually as a 10 percent mix - to create a fuel called gasohol. Ethanol is a renewable resource and ethanol-blended fuels, like gasohol, appear to burn more efficiently in combustion engines. The combustion of one mole of ethanol releases 326.7 kcal of energy.The combustion of one mole of hexane, C6H14, releases 995.0 kcal of energy. How much energy is released during the complete combustion of 380 grams of hexane ?kcalAssuming the same efficiency, would 380 grams of ethanol provide more, less, or the same amount of energy as 380 grams of hexane?
(1) N2(g) + O2(g)2NO(g)...... ΔH° = 181.8 kJ(2) N2(g) + 2O2(g)N2O4(g)......ΔH° = 9.2 kJwhat is the standard enthalpy change for the reaction:(3) 2NO(g) + O2(g)N2O4(g)......ΔH° = ? kJ
A calorimeter is calibrated by mixing 5.00 mL of 0.250 M HC1 and 5.00 mL of 0.250 M NaOH. A temperature rise of 14.26 °C was recorded. Using the same calorimeter, 1.25 mL of 0.500 M CH3COOH was mixed with 2.50 ml of 0.125 M NH3. If the thermometer recorded a temperature rise of 3.35 °C, what is the enthalpy of neutralization of the reaction?

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