Many cigarette lighters contain liquid butane, C.H10(1): 2C.H10(1) + 130z(g) = 8CO2(g)+10H2O(1) Butane has an enthalpy of formation AH°f = -147.6 kJ/mol. Using enthalpies of formation for CO2(g) AH°f = -393.5 kJ/mol, and for H20(1) AH°f = -285.8 kJ/mol, calculate: (a): (b). 22°C to 24 °C, determine the heat capacity of the calorimeter. : the quantity of heat produced when 0.5 g of butane is completely combusted; : If 1.5 g of butane is burned in a bomb calorimeter, and the temperature rises from Atomic mass of hydrogen is 1, and atomic mass of carbon is 12.
Many cigarette lighters contain liquid butane, C.H10(1): 2C.H10(1) + 130z(g) = 8CO2(g)+10H2O(1) Butane has an enthalpy of formation AH°f = -147.6 kJ/mol. Using enthalpies of formation for CO2(g) AH°f = -393.5 kJ/mol, and for H20(1) AH°f = -285.8 kJ/mol, calculate: (a): (b). 22°C to 24 °C, determine the heat capacity of the calorimeter. : the quantity of heat produced when 0.5 g of butane is completely combusted; : If 1.5 g of butane is burned in a bomb calorimeter, and the temperature rises from Atomic mass of hydrogen is 1, and atomic mass of carbon is 12.
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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![Many cigarette lighters contain liquid butane, CAH10(1):
2C4H10(1) + 1302(g) = 8CO2(g)+10H2O(1)
Butane has an enthalpy of formation AH°f = -147.6 kJ/mol. Using enthalpies of formation for
CO2(g) AH°f = -393.5 kJ/mol, and for H2O(1) AH°f = -285.8 kJ/mol, calculate:
(a):
(b).
22°C to 24 °C, determine the heat capacity of the calorimeter.
: the quantity of heat produced when 0.5 g of butane is completely combusted;
: If 1.5 g of butane is burned in a bomb calorimeter, and the temperature rises from
Atomic mass of hydrogen is 1, and atomic mass of carbon is 12.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F418c9341-8d04-457a-aa0b-aec20d9895df%2F370232bd-6a72-4a13-9415-e0db2902ccc5%2Fxsamowp_processed.png&w=3840&q=75)
Transcribed Image Text:Many cigarette lighters contain liquid butane, CAH10(1):
2C4H10(1) + 1302(g) = 8CO2(g)+10H2O(1)
Butane has an enthalpy of formation AH°f = -147.6 kJ/mol. Using enthalpies of formation for
CO2(g) AH°f = -393.5 kJ/mol, and for H2O(1) AH°f = -285.8 kJ/mol, calculate:
(a):
(b).
22°C to 24 °C, determine the heat capacity of the calorimeter.
: the quantity of heat produced when 0.5 g of butane is completely combusted;
: If 1.5 g of butane is burned in a bomb calorimeter, and the temperature rises from
Atomic mass of hydrogen is 1, and atomic mass of carbon is 12.
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