4b. Combustion of 3.500 g of butane gas (C4H10; Mm = 58.12 g/mol) causes a temperature rise (AT) of 29.09°C in a constant-pressure calorimeter that has a heat capacity (Cp) of 5.500 kJ/°C. • Use calorimetry to calculate the heat (q,) released by the combustion of 3.500 g of butane gas in the calorimeter qp = [ Select ] - kJ / 3.500 g of C4H10 • Use the heat (qp) released by the combustion of 3.500 g of butane gas, calculated in part (a) to calculate the change in enthalpy (AHrxn) for the following reaction. (for 1 mole of butane gas): C4H10(9) + 13/2 02(9) →4 CO2(9) + 5 H20(g) AHrxn [ Select ] kJ / mol of C4H10 %3D • Use the heats of formation (AH;°) to calculate the change in enthalpy (AHrxn) for the same reaction. (for 1 mole of butane gas): Heats of Formation: CO2 (g) - A H°f = -393.5 kJ/mol H20(g) - -ΔΗ = -241.8 kJ/mol 02 (g) - A H°f 0.0 kJ/mol C4H10 (9) - A H°f = -125.6 kJ/mol C4H10(9) + 13/2 02(9) → 4 CO2(9) + 5 H20(g) ΔΗη [ Select ] kJ / mol of C4H10 %3D
4b. Combustion of 3.500 g of butane gas (C4H10; Mm = 58.12 g/mol) causes a temperature rise (AT) of 29.09°C in a constant-pressure calorimeter that has a heat capacity (Cp) of 5.500 kJ/°C. • Use calorimetry to calculate the heat (q,) released by the combustion of 3.500 g of butane gas in the calorimeter qp = [ Select ] - kJ / 3.500 g of C4H10 • Use the heat (qp) released by the combustion of 3.500 g of butane gas, calculated in part (a) to calculate the change in enthalpy (AHrxn) for the following reaction. (for 1 mole of butane gas): C4H10(9) + 13/2 02(9) →4 CO2(9) + 5 H20(g) AHrxn [ Select ] kJ / mol of C4H10 %3D • Use the heats of formation (AH;°) to calculate the change in enthalpy (AHrxn) for the same reaction. (for 1 mole of butane gas): Heats of Formation: CO2 (g) - A H°f = -393.5 kJ/mol H20(g) - -ΔΗ = -241.8 kJ/mol 02 (g) - A H°f 0.0 kJ/mol C4H10 (9) - A H°f = -125.6 kJ/mol C4H10(9) + 13/2 02(9) → 4 CO2(9) + 5 H20(g) ΔΗη [ Select ] kJ / mol of C4H10 %3D
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...
Related questions
Question
![4b. Combustion of 3.500 g of butane gas (C4H10; Mm = 58.12 g/mol) causes a temperature rise
(AT) of 29.09°C in a constant-pressure calorimeter that has a heat capacity (C,) of 5.500 kJ/°C.
o Use calorimetry to calculate the heat (q,) released by the combustion of 3.500 g of butane gas
in the calorimeter
Яр
[ Select ]
kJ / 3.500 g of C4H10
o Use the heat (qp) released by the combustion of 3.500 g of butane gas, calculated in part (a) to
calculate the change in enthalpy (AHrxn) for the following reaction. (for 1 mole of butane gas):
C4H10(9) + 13/2 02(9)
→ 4 CO2(9) + 5 H20(g)
AHrxn
[ Select ]
kJ / mol of C4H10
• Use the heats of formation (AH¢°) to calculate the change in enthalpy (AHrxn) for the same
reaction. (for 1 mole of butane gas):
Heats of Formation:
CO2 (g) - A H°f
= -393.5 kJ/mol
H2O(g) - A H°f
= -241.8 kJ/mol
O2 (9) - A H°f
0.0 kJ/mol
C4H10 (g) - A H°f = -125.6 kJ/mol
C4H10(g) + 13/2 02(g)
→ 4 CO2(9) + 5 H20(g)
ΔΗη
[ Select ]
kJ / mol of C4H10](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb99220ad-d702-4943-b904-ec3abe399c73%2Fccc3ab01-7de0-4de4-a483-b4e2a8bd5581%2Flwhfkvi_processed.png&w=3840&q=75)
Transcribed Image Text:4b. Combustion of 3.500 g of butane gas (C4H10; Mm = 58.12 g/mol) causes a temperature rise
(AT) of 29.09°C in a constant-pressure calorimeter that has a heat capacity (C,) of 5.500 kJ/°C.
o Use calorimetry to calculate the heat (q,) released by the combustion of 3.500 g of butane gas
in the calorimeter
Яр
[ Select ]
kJ / 3.500 g of C4H10
o Use the heat (qp) released by the combustion of 3.500 g of butane gas, calculated in part (a) to
calculate the change in enthalpy (AHrxn) for the following reaction. (for 1 mole of butane gas):
C4H10(9) + 13/2 02(9)
→ 4 CO2(9) + 5 H20(g)
AHrxn
[ Select ]
kJ / mol of C4H10
• Use the heats of formation (AH¢°) to calculate the change in enthalpy (AHrxn) for the same
reaction. (for 1 mole of butane gas):
Heats of Formation:
CO2 (g) - A H°f
= -393.5 kJ/mol
H2O(g) - A H°f
= -241.8 kJ/mol
O2 (9) - A H°f
0.0 kJ/mol
C4H10 (g) - A H°f = -125.6 kJ/mol
C4H10(g) + 13/2 02(g)
→ 4 CO2(9) + 5 H20(g)
ΔΗη
[ Select ]
kJ / mol of C4H10
Expert Solution
Step 1
Answer:
Whenever combustion of any hydrocarbon takes place, heat evolves. The value of heat evolved at constant pressure is equal to its enthalpy change and heat evolved at constant volume is equal to its internal energy change.
Step by step
Solved in 4 steps
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY