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32   Use the average bond energies to calculate the ∆H of the reaction:  4H--Cl + O2 → 2H—O—H + 2 Cl—Cl  Data:  ∆H (H-Cl) = 431 kj/mol  ∆H (O-H) = 463 kj/mol  ∆H (O2) = 494 kj/mol  ∆H (Cl-Cl) = 243 kj/mol a. -130 b. -120 c. -150 d. -180

32   Use the average bond energies to calculate the ∆H of the reaction:  4H--Cl + O2 → 2H—O—H + 2 Cl—Cl  Data:  ∆H (H-Cl) = 431 kj/mol  ∆H (O-H) = 463 kj/mol  ∆H (O2) = 494 kj/mol  ∆H (Cl-Cl) = 243 kj/mol a. -130 b. -120 c. -150 d. -180

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter18: Thermodynamics And Equilibrium
Section: Chapter Questions
Problem 18.97QP: When 1.000 g of gaseous butane, C4H10, is burned at 25C and 1.00 atm pressure, H2O(l) and CO2(g) are...
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32   Use the average bond energies to calculate the ∆H of the reaction: 

4H--Cl + O2 → 2H—O—H + 2 Cl—Cl 

Data: 

∆H (H-Cl) = 431 kj/mol 

∆H (O-H) = 463 kj/mol 

∆H (O2) = 494 kj/mol 

∆H (Cl-Cl) = 243 kj/mol

a. -130
b. -120
c. -150
d. -180
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