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:

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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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