Carbon disulfide is a colorless liquid. When pure, it is nearly odorless, but the commercial product smells vile. Carbon disulfide is used in the manufacture of rayon and cellophane. The liquid burns as follows: CS2 (1) + 302 (9) –→ CO2 (g) + 2SO2 (9) Calculate the standard enthalpy change for this reaction using standard enthalpies of formation. AH;(CS2 (1)) = 89.70 kJ/mol AH;(02(9)) = 0 kJ/mol AH¡(CO2(g)) = -393.52 kJ/mol AH¡(SO2(9)) = -296.8 kJ/mol Standard enthalpy change = kJ Submit Answer Try Another Version 10 item attempts remaining
Carbon disulfide is a colorless liquid. When pure, it is nearly odorless, but the commercial product smells vile. Carbon disulfide is used in the manufacture of rayon and cellophane. The liquid burns as follows: CS2 (1) + 302 (9) –→ CO2 (g) + 2SO2 (9) Calculate the standard enthalpy change for this reaction using standard enthalpies of formation. AH;(CS2 (1)) = 89.70 kJ/mol AH;(02(9)) = 0 kJ/mol AH¡(CO2(g)) = -393.52 kJ/mol AH¡(SO2(9)) = -296.8 kJ/mol Standard enthalpy change = kJ Submit Answer Try Another Version 10 item attempts remaining
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
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Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.88QP: The first step in the preparation of lead from its ore (galena, PbS) consists of roasting the ore....
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![Carbon disulfide is a colorless liquid. When pure, it is nearly odorless, but the commercial product smells vile. Carbon disulfide is used in the
manufacture of rayon and cellophane. The liquid burns as follows:
CS2 (1) + 302 (9) –→ CO2 (g) + 2SO2 (9)
Calculate the standard enthalpy change for this reaction using standard enthalpies of formation.
AH;(CS2 (1)) = 89.70 kJ/mol
AH;(02(9)) = 0 kJ/mol
AH¡(CO2(g)) = -393.52 kJ/mol
AH¡(SO2(9))
= -296.8 kJ/mol
Standard enthalpy change =
kJ
Submit Answer
Try Another Version
10 item attempts remaining](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4d149ae6-5772-4fec-96eb-624e06113718%2F37077dc2-3c1c-4796-a6a4-9e6b5a9227e6%2F4d4g05.png&w=3840&q=75)
Transcribed Image Text:Carbon disulfide is a colorless liquid. When pure, it is nearly odorless, but the commercial product smells vile. Carbon disulfide is used in the
manufacture of rayon and cellophane. The liquid burns as follows:
CS2 (1) + 302 (9) –→ CO2 (g) + 2SO2 (9)
Calculate the standard enthalpy change for this reaction using standard enthalpies of formation.
AH;(CS2 (1)) = 89.70 kJ/mol
AH;(02(9)) = 0 kJ/mol
AH¡(CO2(g)) = -393.52 kJ/mol
AH¡(SO2(9))
= -296.8 kJ/mol
Standard enthalpy change =
kJ
Submit Answer
Try Another Version
10 item attempts remaining
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