Thank you again , wow you don't understand your impact you are having on education. All the Engineering/Chem/Physics Undergrads should be watching you . I'm counting on your videos to make me pass my Chemical Thermodynamics Module for my Chemical Engineering Degree. I am optimistic yet partially scared ! :)
One contribution among many which brings the opportunity to learn slightly closer to anyone with an internet connection and the motivation to learn. Thankfully the former is becoming more widespread every day. The latter will prove to be much more of a challenge.
At 2:30 how did you come to the conclusion that dG < 0 indicates to the process being spontaneous? Isn't the relation true for any process since you didn't make the assumption in the beginning that the process spontaneous and mathematically arrived to the conclusion of dG < 0?
We start from the premise that the second law of thermodynamics must be obeyed for the process, thus we have the inequality dS >= dq/T. Using the rest of the derivation here, we arrive at the conclusion that for a system with constant P and T, in order for the second law of thermodynamics to be obeyed, the process must have dG
Notation question/explicit "wordy" interpretation: So in mathematical terms, the total Differential of the sum(U-TS+PV) [aka d(U-TS+PV)] is defined as the differential of G [aka dG]. Which is defined, by name, as the exact differential of Gibbs Energy, such that it is a path independent state function? [subsequently less than or equal to 0 for constant P and T].
I think I agree with this statement for the most part. I would say that G is defined as U-TS+PV, and dU is defined as TdS - PdV, and everything else ends up being true by following the algebra and calculus that results from these two definitions.
A system is isolated when it does not exchange energy or matter with the surroundings. It is closed when it can exchange energy, but not matter with the surroundings. Constant volume removes the ability to do work, but the system may still exchange energy through heat. Saying that a process occurs in a system with constant energy and constant number of particles is equivalent to stating that the system is isolated.
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your videos are gold dude.
Thank you again , wow you don't understand your impact you are having on education. All the Engineering/Chem/Physics Undergrads should be watching you . I'm counting on your videos to make me pass my Chemical Thermodynamics Module for my Chemical Engineering Degree. I am optimistic yet partially scared ! :)
One contribution among many which brings the opportunity to learn slightly closer to anyone with an internet connection and the motivation to learn. Thankfully the former is becoming more widespread every day. The latter will prove to be much more of a challenge.
At 2:30 how did you come to the conclusion that dG < 0 indicates to the process being spontaneous? Isn't the relation true for any process since you didn't make the assumption in the beginning that the process spontaneous and mathematically arrived to the conclusion of dG < 0?
We start from the premise that the second law of thermodynamics must be obeyed for the process, thus we have the inequality dS >= dq/T. Using the rest of the derivation here, we arrive at the conclusion that for a system with constant P and T, in order for the second law of thermodynamics to be obeyed, the process must have dG
Notation question/explicit "wordy" interpretation: So in mathematical terms, the total Differential of the sum(U-TS+PV) [aka d(U-TS+PV)] is defined as the differential of G [aka dG]. Which is defined, by name, as the exact differential of Gibbs Energy, such that it is a path independent state function? [subsequently less than or equal to 0 for constant P and T].
I think I agree with this statement for the most part. I would say that G is defined as U-TS+PV, and dU is defined as TdS - PdV, and everything else ends up being true by following the algebra and calculus that results from these two definitions.
Is the Gibbs free energy change always negative for any process?
Is it the same to say that the process is isolated or that the process takes place at constant energy and constant volume?
A system is isolated when it does not exchange energy or matter with the surroundings. It is closed when it can exchange energy, but not matter with the surroundings. Constant volume removes the ability to do work, but the system may still exchange energy through heat. Saying that a process occurs in a system with constant energy and constant number of particles is equivalent to stating that the system is isolated.
Wow.