A sample of 1.000 g gaseous butane, C4H10, is burned in oxygen at 25°C and 1.00 atm pressure. In the reaction, H20(1) and CO2(g) are the only products and 49.50 kJ of heat was evolved. (i) Determine the molar enthalpy of formation of butane. Given the enthalpies of formation of H;O() is -285.8 kJ/mol and CO2(g) is -393.5 kJ/mol. [Hints: begin with writing the butane combustion equation, take note the heat evolved is for 1.000 g butane] (ii) Determine the AG° for the combustion of 1 mol butane. Use the following data. Substance AG; (kJ/mol) C4H10(g) -17.2 O2(g) H2O(1) -237.1 CO2(g) -394.4 (iii)Determine the AS°for the combustion of 1 mol butane.
A sample of 1.000 g gaseous butane, C4H10, is burned in oxygen at 25°C and 1.00 atm pressure. In the reaction, H20(1) and CO2(g) are the only products and 49.50 kJ of heat was evolved. (i) Determine the molar enthalpy of formation of butane. Given the enthalpies of formation of H;O() is -285.8 kJ/mol and CO2(g) is -393.5 kJ/mol. [Hints: begin with writing the butane combustion equation, take note the heat evolved is for 1.000 g butane] (ii) Determine the AG° for the combustion of 1 mol butane. Use the following data. Substance AG; (kJ/mol) C4H10(g) -17.2 O2(g) H2O(1) -237.1 CO2(g) -394.4 (iii)Determine the AS°for the combustion of 1 mol butane.
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 5.99QE
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![A sample of 1.000 g gaseous butane, C4H10, is burned in oxygen at 25°C and 1.00 atm
pressure. In the reaction, H20(1) and CO2(g) are the only products and 49.50 kJ of heat was
evolved.
(i) Determine the molar enthalpy of formation of butane. Given the enthalpies of formation
of H;0(1) is -285.8 kJ/mol and CO2(g) is -393.5 kJ/mol. [Hints: begin with writing the
butane combustion equation, take note the heat evolved is for 1.000 g butane]
(ii) Determine the AG° for the combustion of 1 mol butane. Use the following data.
Substance
AG; (kJ/mol)
C4H10(g)
-17.2
O2(g)
H2O(1)
-237.1
CO2(g)
-394.4
(iii)Determine the AS°for the combustion of 1 mol butane.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F165bc514-683c-4d5d-b108-223ee84d6e64%2F71c9952f-227d-4155-9dc6-02cbebaa0447%2Fgkw6qbd_processed.png&w=3840&q=75)
Transcribed Image Text:A sample of 1.000 g gaseous butane, C4H10, is burned in oxygen at 25°C and 1.00 atm
pressure. In the reaction, H20(1) and CO2(g) are the only products and 49.50 kJ of heat was
evolved.
(i) Determine the molar enthalpy of formation of butane. Given the enthalpies of formation
of H;0(1) is -285.8 kJ/mol and CO2(g) is -393.5 kJ/mol. [Hints: begin with writing the
butane combustion equation, take note the heat evolved is for 1.000 g butane]
(ii) Determine the AG° for the combustion of 1 mol butane. Use the following data.
Substance
AG; (kJ/mol)
C4H10(g)
-17.2
O2(g)
H2O(1)
-237.1
CO2(g)
-394.4
(iii)Determine the AS°for the combustion of 1 mol butane.
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