Methanol can also be combusted in the presence of oxygen in order to release its energy. 16.0 g of methanol was placed in a bomb calorimeter (with a known heat capacity of 1.37 kJ-K-'), together with 2.50 kg water. 2.2 After methanol was combusted, the temperature of the water increased by 30 °C. Calculate the change in internal energy of methanol (in kJ-mol-')
Methanol can also be combusted in the presence of oxygen in order to release its energy. 16.0 g of methanol was placed in a bomb calorimeter (with a known heat capacity of 1.37 kJ-K-'), together with 2.50 kg water. 2.2 After methanol was combusted, the temperature of the water increased by 30 °C. Calculate the change in internal energy of methanol (in kJ-mol-')
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions
Section: Chapter Questions
Problem 89GQ: Chloroform, CHCl3, is formed from methane and chlorine in the following reaction. CH4(g) + 3 Cl2(g) ...
Related questions
Question
Please answer 2.2 Only.
![2.1
Methanol is an attractive fuel source in a sustainable, green economy. The chemical energy inherent in
methanol can be utilized in a multitude of reactions. Consider the following reaction for the
decomposition of methanol:
2CH;OH(f) → 2CH4(g) + 02(g)
Use Hess' Law to calculate the enthalpy change (in kJ-mol-1) of this reaction, given the following known
thermochemical data:
H20(?) → /202(g) + H2(g)
CH4(g) + H20(g)→ 3H2(g) + CO(g)
2H2 (g) + CO(g) → CH3OH(?)
H20(g) → H20(t)
ДН, — 285.8 k] -тol-1
ДН, — 206.1 k] :тol-1
ΔΗ
ДН, 3D —128.3 k) : тol-1
ΔΗ
Дн, 3D — 44.00 k] -тol-1
[5]
2.2
Methanol can also be combusted in the presence of oxygen in order to release its energy. 16.0 g of methanol
was placed in a bomb calorimeter (with a known heat capacity of 1.37 kJ.K-'), together with 2.50 kg water.
After methanol was combusted, the temperature of the water increased by 30 °C. Calculate the change in
internal energy of methanol (in kJ-mol-')
[5]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe919d4e8-7ddb-410a-93c7-896844b189cf%2Fdd57a9ae-7dbe-4525-9f19-d1672b3690be%2Fvlnd0eq_processed.png&w=3840&q=75)
Transcribed Image Text:2.1
Methanol is an attractive fuel source in a sustainable, green economy. The chemical energy inherent in
methanol can be utilized in a multitude of reactions. Consider the following reaction for the
decomposition of methanol:
2CH;OH(f) → 2CH4(g) + 02(g)
Use Hess' Law to calculate the enthalpy change (in kJ-mol-1) of this reaction, given the following known
thermochemical data:
H20(?) → /202(g) + H2(g)
CH4(g) + H20(g)→ 3H2(g) + CO(g)
2H2 (g) + CO(g) → CH3OH(?)
H20(g) → H20(t)
ДН, — 285.8 k] -тol-1
ДН, — 206.1 k] :тol-1
ΔΗ
ДН, 3D —128.3 k) : тol-1
ΔΗ
Дн, 3D — 44.00 k] -тol-1
[5]
2.2
Methanol can also be combusted in the presence of oxygen in order to release its energy. 16.0 g of methanol
was placed in a bomb calorimeter (with a known heat capacity of 1.37 kJ.K-'), together with 2.50 kg water.
After methanol was combusted, the temperature of the water increased by 30 °C. Calculate the change in
internal energy of methanol (in kJ-mol-')
[5]
Expert Solution
![](/static/compass_v2/shared-icons/check-mark.png)
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 2 steps with 2 images
![Blurred answer](/static/compass_v2/solution-images/blurred-answer.jpg)
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 & Chemical Reactivity](https://www.bartleby.com/isbn_cover_images/9781133949640/9781133949640_smallCoverImage.gif)
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
![Chemistry & Chemical Reactivity](https://www.bartleby.com/isbn_cover_images/9781337399074/9781337399074_smallCoverImage.gif)
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
![General Chemistry - Standalone book (MindTap Cour…](https://www.bartleby.com/isbn_cover_images/9781305580343/9781305580343_smallCoverImage.gif)
General Chemistry - Standalone book (MindTap Cour…
Chemistry
ISBN:
9781305580343
Author:
Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:
Cengage Learning
![Chemistry & Chemical Reactivity](https://www.bartleby.com/isbn_cover_images/9781133949640/9781133949640_smallCoverImage.gif)
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
![Chemistry & Chemical Reactivity](https://www.bartleby.com/isbn_cover_images/9781337399074/9781337399074_smallCoverImage.gif)
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
![General Chemistry - Standalone book (MindTap Cour…](https://www.bartleby.com/isbn_cover_images/9781305580343/9781305580343_smallCoverImage.gif)
General Chemistry - Standalone book (MindTap Cour…
Chemistry
ISBN:
9781305580343
Author:
Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:
Cengage Learning
![Chemistry: The Molecular Science](https://www.bartleby.com/isbn_cover_images/9781285199047/9781285199047_smallCoverImage.gif)
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
![Chemistry: Principles and Practice](https://www.bartleby.com/isbn_cover_images/9780534420123/9780534420123_smallCoverImage.gif)
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781133611097/9781133611097_smallCoverImage.gif)