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

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

Answer both parts

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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