Gibbs Free Energy - Entropy, Enthalpy & Equilibrium Constant K
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- เผยแพร่เมื่อ 6 มิ.ย. 2024
- This video provides a basic introduction into Gibbs Free Energy, Entropy, and Enthalpy. It explains how to calculate the equilibrium constant K given the standard free energy change of a reaction and so much more.
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The link doesn't work for me , can you reshare it please 🙏🏼
@@assilmarref4846 you need to become a patreon which costs money
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Hey man, I used your videos to study for my MCAT back in 2018, now I'm currently studying for my Step 1 exam in medical school. glad to see you are still pumping out new videos. Thanks for all your good work!
wait......why are you doing chemistry calculations in medical school???
@@aojbooker8650 you can go to med school as a chemistry major, also you need to take gen chem and ochem for med school soooooo
@@valorantyie9820 yes of course you can go to medical school as a chemistry major.....but as far as I understand he is doing chemistry calculations while already being in medical school, which is why I am confused. I'm not sure why in the world he would need to understand Gibbs free energy as a med student. And no I live in Canada so I do not need to take specific chem classes to go to most medical schools. However most medical schools do indeed have a chemistry requirement. For example a medical school could prerequire two introductory chemistry classes in which case I could do ochem and bio chem and completely ignore gen chem.
@@aojbooker8650 perhaps he's studying with other videos regarding his subject and not specifically Chem and this was one of the users most recent videos and that's why he said he's glad he's still posting under this specific vid regardless what subject it is
@@aojbooker8650 Wow you can take OCHEM and BIOCHEM without gen chem. Thats interesting.
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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.🧐
Hola, muchas gracias, lamentablemente, no hay videos en español que comenten sobre la formula de energia libre de Gibbs en equilibrio, me has explicado a pesar de mi bajo nivel de ingles, he podido entender todo, te agradezco enormemente, me ayudas con Bioquimica, Greetings from Chile
this channel is doing gods work
Indeed, you are truly godsend!
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.
I wish I could read what you have written because I love Korean language so so much
@@dragonartgroup6982 may be now you can read
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@@dragonartgroup6982 how's Google translate helping you out
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Haven't paid attention in the last 2 lectures, 45min got me right.
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Same
The timing of this is…pheNOMenal
Just want to say thank you man
I have my chem final tomorrow, thnx
Very useful
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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?
You are absolutely right. The discussed 3 conditions are actually 3 possibilities at equilibrium
At equilibrium, the constant K, the rate is constant, and the same, but the concentrations are not the same, they are just constant.
Thanks for sharing this 🙏
You are just amazing thank u
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?
Assuming the reaction is endothermic in the forward direction, the system requires work. Hence, the reaction is non-spontaneous meaning the Entropy of the universe is negative. If you watch this video, you will see the answers for yourself: th-cam.com/video/lN66F9V7-_Q/w-d-xo.html
Thank you!!!! God blessss
On the third problem, on the dealta S reaction, why were the reactants minus each other to get 20 J/mol?
Thanks for nice lecture. You explained well. Can you please explain "why water boils at 100°C?
That’s just how the Celsius system works. At 0 degrees Celsius, water freezes
@@advantphoenix7892 no one can explain.anything. They have merely observed repeated phenomenon.
100C is when the intermolecular bonds of liquid water are torn by the movement of the thermal energy causing particularly to fly away now no longer attached to the main water mass, now it’s a gas!
Can anyone tell me which reference tables are used to get enthalpy and entropy of the reactants and products pls pls
How could we assume that Kp equals to Kc with the question number 9?
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?
Thanks 😊
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Watching this at 1 am I’ve got a Chem test tomorrow and have no idea what I’m doing lol😭😭
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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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Can I see the picture of the tutor
i think you'll find for the starting question that the answer is E. None of the above is false - since D. is false.
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In the first question you actually also have that "E" is a false statement :-)
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from where we get the 298 ?
To convert to Kelvin, add 273 (technically 273.15 but the extra decimals tend to be negligible) to your Celsius temperature. 298 Kelvin is a very common temperature in chemistry, it’s the standard temperature value (that or 25° Celsius, they’re the same thing)
The way he says Joules reminds me of Jules in Euphoria
On problem 10 why did you do R is 8.314. I thought R was 4.184???
Nope 8.314
The answer of 5 no question is 24 not -36. please check it.
those gibbs value are for the reaction not the compounds. As a result, once the equations are rearranged instead of subtracting products and reactants (which i am guessing u did) to obtain the gibbs value for the final equation you need to just add those two earlier reactions.
40:56
the unit for free energy change is kj/mol . you forgot the mol
It is energy change
wait where did he get 273? at the part of the 25-degree celsius?
what are you talking about? what's the time stamp? are you talking about when he found the boiling point of bromine? he subtracted 273 degrees K in order to get the temperature in C
273.15 K is used in dimensional analysis to move between temperature units Kelvin, Celsius, and Fahrenheit, eg: 15 °C can be converted to K by (15+273.15) = 288.15 K.
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languages of the same thing, pretty cool to learn if ever working with someone or gentile that talks in different meausment languages, im more of ev to mole, see ya
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2024
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Thank you.
Fucking hate chemistry