Bond Energy and Diagrams

.pdf

School

Woodland High School *

*We aren’t endorsed by this school

Course

7352

Subject

Chemistry

Date

Nov 24, 2024

Type

pdf

Pages

Uploaded by zizaa222

Zahra .F. Jabbar Bond Energy and Diagrams 1. How much energy is contained in each of the following? (3 marks) 1. 3 moles of chlorine molecules - 242Kj x 2 mol x 3 mol - 1452 kj 2. 5 moles of ammonia molecules - 389 kj x 3 mol x 5 mol = 5835kj 3. 4.8 moles of propane- 19152 kj 2. Calculate the overall ΔH for each reaction. Make an energy diagram for the heat formation of one mole of each of the following substances. (2 marks for ΔH, 1 mark for diagram) = 9 marks) 1.

Zahra .F. Jabbar = 140 kj/mol 2. 3.

Zahra .F. Jabbar 3. If the change in enthalpy for carbon monoxide (CO) is -104.5 kJ/mol, and that of carbon dioxide (CO 2 ) is -392.92 kJ/mol, what can we conclude about the stability of these two substances? (1 mark) 4. Calculate the change in enthalpy for the following reactions. Make sure each equation is balanced. (3 marks each = 12 marks) 1. = -1440 KJ mol

Your preview ends here

Eager to read complete document? Join bartleby learn and gain access to the full version

Access to all documents
Unlimited textbook solutions
24/7 expert homework help

Zahra .F. Jabbar 2. 3. 4. 5. Find the enthalpy for the complete combustion of methanol. (4 marks) 6. Methylhydrazine is commonly used as a liquid rocket fuel. Its combustion is indicated by the following reaction. 1. Balance this equation. (1 mark) 2. Calculate ΔH for this reaction. (3 marks) 7. The heat of combustion of hydrogen gas per gram is about 2.5 times that of natural gas. The main component of natural gas is methane gas. Also, the combustion of hydrogen is “cleaner” than that of natural gas, since the only product is water. Thus, it seems a likely choice for a major fuel source in the future. Prove that the heat of combustion of hydrogen per gram is about 2.5 times that of natural gas. Begin by calculating the heat associated with the combustion of each fuel in kJ/g of fuel. (4 marks)

Recommended textbooks for you

Chemistry & Chemical Reactivity

Chemistry

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:Cengage Learning

Introductory Chemistry: A Foundation

Chemistry

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Cengage Learning

Chemistry

ISBN:9781305957404

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

Publisher:Cengage Learning

SEE MORE TEXTBOOKS

Recommended textbooks for you

Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning