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In some parts of the world, butadiene was produced from ethanol, C2H6O by the unbalanced reaction: C2H60 (g) → C4H6 (g) + H20 (g) + H2 (g) 1. Balance the above reaction. I'd like you to determine whether this reaction is exo- or endothermic, but you need more information first. The following questions will walk you through this process. 2. Given the reaction and thermochemical data below, use Hess' Law to calculate A H,xn for the gas-phase combustion of butadiene. 11 O2 (g) = ? kJ C4H6 (g) + 4 CO2 (g) + 3 H20(1) - 2 H20 (g) A H; = -484 kJ 2 H2 (g) + O2 (g) + 6 02 (9) 4 CO2 (g) + 4 H20 (g) AHxn =-2527 kJ C4H8 (g) AHixn = +132 kJ C4H8 (g) C4H6 (g) + H2 (g) AHvap = +41 kJ H20(1) H20 (g)

In some parts of the world, butadiene was produced from ethanol, C2H6O by the unbalanced reaction: C2H60 (g) → C4H6 (g) + H20 (g) + H2 (g) 1. Balance the above reaction. I'd like you to determine whether this reaction is exo- or endothermic, but you need more information first. The following questions will walk you through this process. 2. Given the reaction and thermochemical data below, use Hess' Law to calculate A H,xn for the gas-phase combustion of butadiene. 11 O2 (g) = ? kJ C4H6 (g) + 4 CO2 (g) + 3 H20(1) - 2 H20 (g) A H; = -484 kJ 2 H2 (g) + O2 (g) + 6 02 (9) 4 CO2 (g) + 4 H20 (g) AHxn =-2527 kJ C4H8 (g) AHixn = +132 kJ C4H8 (g) C4H6 (g) + H2 (g) AHvap = +41 kJ H20(1) H20 (g)

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter5: Thermochemistry
Section: Chapter Questions
Problem 5.36QE: When lightning strikes, the energy can force atmospheric nitrogen and oxygen to react to make NO:...
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In some parts of the world, butadiene was produced from ethanol, C2H&O by the unbalanced reaction: C2H60 (g) → C4H6 (g) + H20 (g) + H2 (g) 1. Balance the above reaction. I'd like you to determine whether this reaction is exo- or endothermic, but you need more information first. The following questions will walk you through this process. 2. Given the reaction and thermochemical data below, use Hess' Law to calculate A H,xn for the gas-phase combustion of butadiene. 11 O2 (g) = ? kJ C4H6 (g) + 4 CO2 (g) + 3 H20(1) - 2 H2O(g) A H; = -484 kJ 2 H2 (g) + O2 (g) + 6 02 (9) 4 CO2 (g) + 4 H2O(g) AHxn =-2527 kJ C4H8 (g) AHxn =+132 kJ C4H8 (g) C4H6 (g) + H2 (g) AHvap = +41 kJ H20 (1) H2O (g)
Transcribed Image Text:In some parts of the world, butadiene was produced from ethanol, C2H&O by the unbalanced reaction: C2H60 (g) → C4H6 (g) + H20 (g) + H2 (g) 1. Balance the above reaction. I'd like you to determine whether this reaction is exo- or endothermic, but you need more information first. The following questions will walk you through this process. 2. Given the reaction and thermochemical data below, use Hess' Law to calculate A H,xn for the gas-phase combustion of butadiene. 11 O2 (g) = ? kJ C4H6 (g) + 4 CO2 (g) + 3 H20(1) - 2 H2O(g) A H; = -484 kJ 2 H2 (g) + O2 (g) + 6 02 (9) 4 CO2 (g) + 4 H2O(g) AHxn =-2527 kJ C4H8 (g) AHxn =+132 kJ C4H8 (g) C4H6 (g) + H2 (g) AHvap = +41 kJ H20 (1) H2O (g)
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