A commercial process for preparing ethanol, C,H50H(9) , involves the process of passing ethylene gas, C„H4(9), and steam, H,0(9) over a catalyst (to increase the reaction rate). The reaction is given below: + H,0 -H, H-ċ- AHpn = kJ H ÓH a) Use Bond Energies to calculate the change in enthalpy (AHxn) for this reaction: Bond Bond Energies C-C 346 kJ/mol C=C 602 kJ/mol C-H 411 kJ/mol C-O 358 kJ/mol O-H 459 kJ/mol AHxn = E B.E. (bonds broken) - E B.E. (bonds formed) • The sum of the Bond Energies Broken: [ Select ] v kJ • The sum of the Bond Energies Formed: [ Select) kJ • Enthalpy of Reaction(AHxn) (from Bond Energies): [ Select ] kJ b) Use the Heats of Formation (AH÷ °) to calculate the change in enthalpy (AHxn) for this reaction: ΔΗ.-Σ (n. ΔΗ ') productsΣ (n ο Δ Η; )reactants CH4(9) A HĘ ° = + 52.47 kJ/mol A H ° = - 241.8 kJ/mol C„H5OH(@) A H¢ ° = - 235.1 kJ/mol • Enthalpy of Reaction(AHxn) (from Heats of Formation ): [ Select ] v kJ
A commercial process for preparing ethanol, C,H50H(9) , involves the process of passing ethylene gas, C„H4(9), and steam, H,0(9) over a catalyst (to increase the reaction rate). The reaction is given below: + H,0 -H, H-ċ- AHpn = kJ H ÓH a) Use Bond Energies to calculate the change in enthalpy (AHxn) for this reaction: Bond Bond Energies C-C 346 kJ/mol C=C 602 kJ/mol C-H 411 kJ/mol C-O 358 kJ/mol O-H 459 kJ/mol AHxn = E B.E. (bonds broken) - E B.E. (bonds formed) • The sum of the Bond Energies Broken: [ Select ] v kJ • The sum of the Bond Energies Formed: [ Select) kJ • Enthalpy of Reaction(AHxn) (from Bond Energies): [ Select ] kJ b) Use the Heats of Formation (AH÷ °) to calculate the change in enthalpy (AHxn) for this reaction: ΔΗ.-Σ (n. ΔΗ ') productsΣ (n ο Δ Η; )reactants CH4(9) A HĘ ° = + 52.47 kJ/mol A H ° = - 241.8 kJ/mol C„H5OH(@) A H¢ ° = - 235.1 kJ/mol • Enthalpy of Reaction(AHxn) (from Heats of Formation ): [ Select ] v kJ
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
Concept explainers
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Question
Hi! This question was answered before, but it was incorrect. Could it be answered again? Thanks!
![A commercial process for preparing ethanol, C2H;OH(g) , involves the process of passing ethylene gas, C,H4(g), and steam, H,0(g) over a catalyst (to increase the reaction
rate).
The reaction is given below:
H
H
H,
H*.
+ H,0
H-Ć-Ć-H
AHxn =
kJ
H
H.
H
OH
a) Use Bond Energies to calculate the change in enthalpy (AHxn) for this reaction:
Bond
Bond Energies
C-C
346 kJ/mol
C=C
602 kJ/mol
C-H
411 kJ/mol
C-O
358 kJ/mol
О-Н
459 kJ/mol
AHrxn = E B.E. (bonds broken) - E B.E. (bonds formed)
• The sum of the Bond Energies Broken:
[ Select ]
v kJ
• The sum of the Bond Energies Formed:
[ Select]
v kJ
Enthalpy of Reaction(AHrxn) (from Bond Energies):
[ Select ]
kJ
b) Use the Heats of Formation (AH°) to calculate the change in enthalpy (AHxn) for this reaction:
ΔΗη Σ (n. ΔΗ; ) products -Σ (n ο ΔΗ, Ό )reactants
CHa(9)
A Hf ° = + 52.47 kJ/mol
A Hf ° = - 241.8 kJ/mol
C2H5OH(9) A Hf ° = - 235.1 kJ/mol
Enthalpy of Reaction(AHrxn) (from Heats of Formation ):
[ Select ]
v kl](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F66173c1a-f883-4b2a-9c4a-34112153fb2f%2F039e6a17-2c9d-46fd-8217-79254e99f2a3%2Fr73eshr_processed.png&w=3840&q=75)
Transcribed Image Text:A commercial process for preparing ethanol, C2H;OH(g) , involves the process of passing ethylene gas, C,H4(g), and steam, H,0(g) over a catalyst (to increase the reaction
rate).
The reaction is given below:
H
H
H,
H*.
+ H,0
H-Ć-Ć-H
AHxn =
kJ
H
H.
H
OH
a) Use Bond Energies to calculate the change in enthalpy (AHxn) for this reaction:
Bond
Bond Energies
C-C
346 kJ/mol
C=C
602 kJ/mol
C-H
411 kJ/mol
C-O
358 kJ/mol
О-Н
459 kJ/mol
AHrxn = E B.E. (bonds broken) - E B.E. (bonds formed)
• The sum of the Bond Energies Broken:
[ Select ]
v kJ
• The sum of the Bond Energies Formed:
[ Select]
v kJ
Enthalpy of Reaction(AHrxn) (from Bond Energies):
[ Select ]
kJ
b) Use the Heats of Formation (AH°) to calculate the change in enthalpy (AHxn) for this reaction:
ΔΗη Σ (n. ΔΗ; ) products -Σ (n ο ΔΗ, Ό )reactants
CHa(9)
A Hf ° = + 52.47 kJ/mol
A Hf ° = - 241.8 kJ/mol
C2H5OH(9) A Hf ° = - 235.1 kJ/mol
Enthalpy of Reaction(AHrxn) (from Heats of Formation ):
[ Select ]
v kl
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 3 steps with 4 images
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