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Butane, C4H10, is the gas used for gas barbecues. Given the following values for enthalpy of formation at 25°C: ΔΗ, = -125.6 Answer: C4H10 (g): kJ/mol H₂O (g): kJ/mol CO₂ (g): kJ/mol a) Calculate the enthalpy of reaction at 25°C for the burning of butane: kJ ΔΗ° = -241.8 ΔΗ° = -393.5 2 C4H10 (9) + 13 O₂ (g) - 8 CO₂ (g) + 10 H₂O (g) kJ/mol b) Calculate the quantity of energy (in kJ) released when 525 g of butane is burned: Answer:

Butane, C4H10, is the gas used for gas barbecues. Given the following values for enthalpy of formation at 25°C: ΔΗ, = -125.6 Answer: C4H10 (g): kJ/mol H₂O (g): kJ/mol CO₂ (g): kJ/mol a) Calculate the enthalpy of reaction at 25°C for the burning of butane: kJ ΔΗ° = -241.8 ΔΗ° = -393.5 2 C4H10 (9) + 13 O₂ (g) - 8 CO₂ (g) + 10 H₂O (g) kJ/mol b) Calculate the quantity of energy (in kJ) released when 525 g of butane is burned: Answer:

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter5: Thermochemistry
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Problem 80E: Ethanol, C2H5OH, is used as a fuel for motor vehicles, particularly in Brazil. (a) Write the...
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Butane, C4H10, is the gas used for gas barbecues. Given the following values for enthalpy of formation at 25°C: ΔΗ, = -125.6 Answer: C4H10 (g): kJ/mol H₂O (g): kJ/mol CO₂ (g): kJ/mol a) Calculate the enthalpy of reaction at 25°C for the burning of butane: kJ ΔΗ, = -241.8 kJ/mol ΔΗ, = -393.5 2 C4H10 (9) + 13 O₂ (g) - 8 CO₂ (g) + 10 H₂O (g) b) Calculate the quantity of energy (in kJ) released when 525 g of butane is burned: Answer:
Transcribed Image Text:Butane, C4H10, is the gas used for gas barbecues. Given the following values for enthalpy of formation at 25°C: ΔΗ, = -125.6 Answer: C4H10 (g): kJ/mol H₂O (g): kJ/mol CO₂ (g): kJ/mol a) Calculate the enthalpy of reaction at 25°C for the burning of butane: kJ ΔΗ, = -241.8 kJ/mol ΔΗ, = -393.5 2 C4H10 (9) + 13 O₂ (g) - 8 CO₂ (g) + 10 H₂O (g) b) Calculate the quantity of energy (in kJ) released when 525 g of butane is burned: Answer:
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