Gibbs Free Energy - Entropy, Enthalpy & Equilibrium Constant K 

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Dear Organic Chemistry Tutor, First of all, many sincere thanks for your efforts! A. There is ONLY ONE BASIC, fundamental Energy Conservation and Transformation Law. It is definitely unique and conceptually indivisible delivering two logically joint concepts - these are Energy Conservation - and Energy Transformation. Still, a more-then-100-years-old conceptual failure has brought us to two separate thermodynamic laws - but this has nothing in common with the actual physics. To come back, they have coined two more fake thermodynamic laws, employed the Probability Theory + Mathematical Statistics, and this has helped formulate the Quantum Mechanics, which is thus a basically metaphysical conceptual construction and thus ought to be only restrictedly fruitful. B. By dividing the basically indivisible law, you are telling about Combinatorics, you are touching Probability Theory, you are even stepping back to Thermodynamics for a while, but... You are NOT answering the poser: WHAT IS ENTROPY, sorry! 1. In the formula S = kB * ln(Ω) you imply, Ω means not a "Huge Number of Microstates", not "Probability", which numerically ranges between [0,1], not even "Wavefunction", which ought to be a purely metaphysical notion, as it is... In effect, Ω ought to be a simplistic algebraic function of Lord Kelvin's Absolute Temperature. This result has been published 100 years ago in JACS. 2. WHAT-ENTROPY-IS-poser has been answered not by Clausius, not by Boltzmann, etc., but by Goethe, who has introduced Mephistopheles, the philosophical embodiment of ENTROPY. 3. Newton did basically know WHAT ENTROPY IS - A Counteraction. 4. That Counteractions do not grow to infinity with the growing Actions, but MUST reach their MAXIMUM values, is the result by Nicky Carnot formalized by Clausius... 5. In effect, Gibbs Energy formula renders implicit the interplay among ALL the relevant Actions (the Enthalpic term) and ALL the Counteractions (the Entropic term). 6. The standard approach you are reporting about is OK for the implicit Enthalpy-Entropy picture, employing it for studying reaction mechanism details is likewise eating soup with fork.🧐

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깁스 자유에너지, 엔트로피, 엔탈피 이름만 들어도 무슨 저런 어려운 이름이 다있어라는 생각이 들정도로 친숙해지기 쉽지 않은 단어처럼 느껴지지만 자연상태에서 이러나는 자연스로운 현상임을 이 영상을 통해 인식한 이후에는 한결 이 개념들에 대해 친숙해 진 것 같습니다.

Thanks 😊

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I really enjoy the videos. I have a question on this one. You discuss K the eq, constant, and say K=1 at equilibrium. Is that not false? K can equal any number of value at equilibrium. I understand that we can use whether K< or > 1 to determine whether it is reactant or product favored, but a K=1 would only tell us the concentrations are equal, not the rate of reaction. Am I misunderstanding this?

Exam in 13 minutes

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Thanks for nice lecture. You explained well. Can you please explain "why water boils at 100°C?

If u have an endothermic reaction (delta H is positive) like H2 + I2 --> 2HI can you say whether the entropy rises or decreases and whether the reaction could be spontaneous?

Watching this at 1 am I’ve got a Chem test tomorrow and have no idea what I’m doing lol😭😭

How could we assume that Kp equals to Kc with the question number 9?

On the third problem, on the dealta S reaction, why were the reactants minus each other to get 20 J/mol?

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Can anyone tell me which reference tables are used to get enthalpy and entropy of the reactants and products pls pls

Can anyone explain for a combustion reaction where ΔSsystem is positive and ΔH is negative, even though I know the reaction will always be spontaneous, how do I determine if lowering the temperature makes it more or less spontaneous? If ΔG=ΔH-TΔS then lowering the temperature would make ΔG less negative and less spontaneous but since ΔS surroundings=-ΔH/T approaches infinity as temperature decreases then the entropy of the universe contradicts this and implies that lowering the temperature makes the reaction more spontaneous. So if I wanted to know if lowering the temperature makes the reaction more or less spontaneous which do I look at, ΔG or ΔS of the universe. Why are they contradicting each other?

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i think you'll find for the starting question that the answer is E. None of the above is false - since D. is false.

how did you get the negative -109.7?

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One question if someone might be able to help: I came across the terms "desolvation penalty" and "rigidization penalty" in binding events which were both labelled as entropic penalties. The second I understand, as rigidization decreases the number of microstates of the system. But how does dehydration present a positive entropy term? Shouldn't the release of water in the system be a favoured entropic event, by allowing for more degrees of freedome as compared to water being forced in an order manner around an undefined molecular surface? Would be glad if someone could help out. All the best!

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In the first question you actually also have that "E" is a false statement :-)

The answer of 5 no question is 24 not -36. please check it.

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from where we get the 298 ?

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On problem 10 why did you do R is 8.314. I thought R was 4.184???

Hey

the unit for free energy change is kj/mol . you forgot the mol

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Organic Chem tutor>>>3 weeks of useless lectures

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