Calculate the enthalpy change for the dissolution of (NH4)2SO4(s) using the enthalpy of formation data provided below: (remember to write the balanced equation for the dissolution reaction including state symbols). Explain how the value obtained here might be different from the value obtained using calorimetry. Compound Enthalpies of formation (kJmol-1) (NH4)2SO4 (s) -1380.9 (NH4)+ (aq) -143.5 (SO4)2- (aq) -1009.0
Calculate the enthalpy change for the dissolution of (NH4)2SO4(s) using the enthalpy of formation data provided below: (remember to write the balanced equation for the dissolution reaction including state symbols). Explain how the value obtained here might be different from the value obtained using calorimetry. Compound Enthalpies of formation (kJmol-1) (NH4)2SO4 (s) -1380.9 (NH4)+ (aq) -143.5 (SO4)2- (aq) -1009.0
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
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
Section5.8: Product- Or Reactant-favored Reactions And Thermodynamics
Problem 1.1ACP: The standard enthalpies of formation of KNO3(s) and K2S(s) are 494.6 kJ/mol and 376.6 kJ/mol,...
Related questions
Question
Calculate the enthalpy change for the dissolution of (NH4)2SO4(s) using the enthalpy of formation data provided below: (remember to write the balanced equation for the dissolution reaction including state symbols). Explain how the value obtained here might be different from the value obtained using calorimetry.
Compound |
Enthalpies of formation (kJmol-1) |
(NH4)2SO4 (s) |
-1380.9 |
(NH4)+ (aq) |
-143.5 |
(SO4)2- (aq) |
-1009.0 |
Expalin
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 2 steps with 2 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 & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
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
Physical Chemistry
Chemistry
ISBN:
9781133958437
Author:
Ball, David W. (david Warren), BAER, Tomas
Publisher:
Wadsworth Cengage Learning,
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning