1 1 a. Use the data collected by experiment to calculate a molar enthalpy of reaction for methanol. (2600g) (4.1843/g") C219-20.5) = 805003 = 80.5 KJ Answer: 4.389 32.02g/mol = 1362mol [-598 kJ/mol ] -805kJ <- O.1362 mol Answer: b. Use the value calculated in question 4.a to calculate the standard molar enthalpy of formation for methanol [-279.1 kJ/mol or -367.1 kJ/mol, only one is correct!] -598 kJ/mol CH₂OH+3/202-32H₂0 CH 30H C-393.5)+2mol C-285.8)-(597.9) = -367.1 kJ c. Calculate a percentage difference between the value calculated in question 4.b and the value for the standard molar enthalpy of formation for methanol shown in your Chemistry 30 Data Booklet (This can be found posted on Moodle - you should print off a copy and keep it handy for all of your assignments, if you have not already done so) Standard molar enthalpy of formation =CH₂OH(1) -239.2 for methanol [ 53.5 % ]
1 1 a. Use the data collected by experiment to calculate a molar enthalpy of reaction for methanol. (2600g) (4.1843/g") C219-20.5) = 805003 = 80.5 KJ Answer: 4.389 32.02g/mol = 1362mol [-598 kJ/mol ] -805kJ <- O.1362 mol Answer: b. Use the value calculated in question 4.a to calculate the standard molar enthalpy of formation for methanol [-279.1 kJ/mol or -367.1 kJ/mol, only one is correct!] -598 kJ/mol CH₂OH+3/202-32H₂0 CH 30H C-393.5)+2mol C-285.8)-(597.9) = -367.1 kJ c. Calculate a percentage difference between the value calculated in question 4.b and the value for the standard molar enthalpy of formation for methanol shown in your Chemistry 30 Data Booklet (This can be found posted on Moodle - you should print off a copy and keep it handy for all of your assignments, if you have not already done so) Standard molar enthalpy of formation =CH₂OH(1) -239.2 for methanol [ 53.5 % ]
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter5: Thermochemistry
Section: Chapter Questions
Problem 5.99QE
Related questions
Question
Can you do question c please
![1
a. Use the data collected by experiment to calculate a molar enthalpy of reaction for
methanol.
1
Answer:
4.389
32.02g/mol
= 1362mol
b. Use the value calculated in question 4.a to calculate the standard molar enthalpy of
formation for methanol
[-279.1 kJ/mol or -367.1 kJ/mol, only one is correct!]
Answer:
[-598 kJ/mol ]
-80.5kJ = -598 kJ/mol
0.1362 mol
CH₂OH+3/202-32H₂0 CH3OH
C-393.5)+2mol C-285.8)-(597.9)
= -367.1 kJ
C2600g)c4.189J/g)
C21.9-20.5) = 905003
= 80.5 KJ
Answer:
c. Calculate a percentage difference between the value calculated in question 4.b and
the value for the standard molar enthalpy of formation for methanol shown in your
Chemistry 30 Data Booklet (This can be found posted on Moodle - you should print
off a copy and keep it handy for all of your assignments, if you have not already done
so)
Standard molar enthalpy of formation =CH₂OH(1) -239.2
[ 53.5 % ]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb5fdd233-e947-4d5f-a3c0-4edca06f47b3%2F24455d7a-127e-47a8-8095-e9ebc045c992%2F8qftby7_processed.jpeg&w=3840&q=75)
Transcribed Image Text:1
a. Use the data collected by experiment to calculate a molar enthalpy of reaction for
methanol.
1
Answer:
4.389
32.02g/mol
= 1362mol
b. Use the value calculated in question 4.a to calculate the standard molar enthalpy of
formation for methanol
[-279.1 kJ/mol or -367.1 kJ/mol, only one is correct!]
Answer:
[-598 kJ/mol ]
-80.5kJ = -598 kJ/mol
0.1362 mol
CH₂OH+3/202-32H₂0 CH3OH
C-393.5)+2mol C-285.8)-(597.9)
= -367.1 kJ
C2600g)c4.189J/g)
C21.9-20.5) = 905003
= 80.5 KJ
Answer:
c. Calculate a percentage difference between the value calculated in question 4.b and
the value for the standard molar enthalpy of formation for methanol shown in your
Chemistry 30 Data Booklet (This can be found posted on Moodle - you should print
off a copy and keep it handy for all of your assignments, if you have not already done
so)
Standard molar enthalpy of formation =CH₂OH(1) -239.2
[ 53.5 % ]
Expert Solution
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 3 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: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
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: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
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
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: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:
9781938168390
Author:
Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:
OpenStax
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
World of Chemistry
Chemistry
ISBN:
9780618562763
Author:
Steven S. Zumdahl
Publisher:
Houghton Mifflin College Div