If the entropy change for the reaction is ∆Ssys = −308.6 J mol-1 K-1 at 298,15 K, what value must ∆Hsys have for the reaction to be spontaneous?
If the entropy change for the reaction is ∆Ssys = −308.6 J mol-1 K-1 at 298,15 K, what value must ∆Hsys have for the reaction to be spontaneous?
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter13: Spontaneous Processes And Thermodynamic Equilibrium
Section: Chapter Questions
Problem 22P: Use data from Appendix D to calculate the standardentropy change at 25°C for the reaction...
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Question
Ammonium Nitrate is a fertilizer that can be made by combining nitric acid and ammonia as follows:
HNO3(g) + NH3(g) à NH4NO3(s)
The change in entropy for the reaction is
∆Ssys =∑n∆Sprod − ∑ m∆Sreact
The change in the entropy for the surroundings is
∆Ssurr =−∆Hsys /T
and the change to the entropy of the universe is
∆Suniv = ∆Ssys +∆Ssurr
If the entropy change for the reaction is
∆Ssys = −308.6 J mol-1 K-1
at 298,15 K, what value must ∆Hsys have for the reaction to be spontaneous?
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