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Ch.19 - Chemical Thermodynamics
All textbooksBrown 14th EditionCh.19 - Chemical ThermodynamicsProblem 53a
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Chapter 19, Problem 53a

(a) For a process that occurs at constant temperature, does the change in Gibbs free energy depend on changes in the enthalpy and entropy of the system?

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Hello everyone. So in this video we want to see if the statement is true or false. The statement reads the change in Gibbs free energy is determined by the system's entropy and entropy at constant temperature. So our Gibbs free energy equation is that the delta G. Is equal to our delta H minus the temperature multiplied by our delta S. So we have said in the problem that the T. Is a constant value, so that means that the only contributing factors affects our delta G is going to be. So let's see affecting factors is going to include our delta H and R delta us delta H. Being our entropy delta. S. Being our entropy. So therefore the statement is going to be true. And this right here is going to be my final answer for this problem. Thank you all so much for watching.
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Textbook Question
The standard entropies at 298 K for certain group 4A elements are: C(s, diamond) = 2.43 J>mol@K, Si1s2 = 18.81 J>mol@K, Ge1s2 = 31.09 J>mol@K, and Sn1s2 = 51.818 J>mol@K. All but Sn have the same (diamond) structure. How do you account for the trend in the S° values?
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