4. For the reaction below: a. How many non-polar and polar bonds are in the reactants? b. How many non-polar and polar bonds are in the products? c. What is the enthalpy (AH) of this reaction? What is your evidence for this response? d. What is the entropy (AS) of this reaction? What is your evidence for this response? e. Is the reaction below spontaneous/non-spontaneous and endergonic/exergonic? f. Is carbon being oxidized or reduced? Why?

4. For the reaction below: a. How many non-polar and polar bonds are in the reactants? b. How many non-polar and polar bonds are in the products? c. What is the enthalpy (AH) of this reaction? What is your evidence for this response? d. What is the entropy (AS) of this reaction? What is your evidence for this response? e. Is the reaction below spontaneous/non-spontaneous and endergonic/exergonic? f. Is carbon being oxidized or reduced? Why?

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter10: Entropy And The Second Law Of Thermodynamics

Section: Chapter Questions

Problem 10.33PAE: Limestone is predominantly CaCO3, which can undergo the reaction CaCO3(s)CaO(s)+CO2(g). We know from...

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Limestone is predominantly CaCO3, which can undergo the reaction CaCO3(s)CaO(s)+CO2(g). We know from experience that this reaction is not spontaneous, yet S for the reaction is positive. How can the second law of thermodynamics explain that this reaction is not spontaneous?