Absolutely incredible!!! I study physics in Romania and the system here is based on mechanical learning, no logic thinking, just learn like a computer. You just saved me man!!!
Great to follow. remark: Going from R to kB implies that you go from an ensemble of particles to an average particle. Essential is that the properties G, S, H, P, T are average values that do not change in time at equilibrium.
Hi you said enthalpy is with constant pressure then how in the equation of enthalpy we are getting dp which is change of pressure so shouldn't that dp be zero??
Great explanation! Was wondering however the physical significance of our exact differential equations. For example dH= TdS +VdP, but we said that change in P for enthalpy is 0, so what's going on here?
So the purpose of defining enthalpy is so that we can have a change in an exact quantity that is good for circumstances in which pressure is constant. In the case of internal energy, dU = TdS + pdV the variables S and V directly correspond to a change in U, hence measuring the internal energy U is great for processes with constant volume and entropy, but less good for processes with constant pressure. Defining enthalpy H = U + PV eliminates this, and we find that change in pressure dP corresponds directly to a change in enthalpy dH. Combining this with the first law of thermodynamics we can actually equate the change in heat energy, dQ (which is not an exact differential), to a change in enthalpy dH (which is an exact differential), provided that the pressure is constant (dp = 0). Hope that helps! :)
@@pazzy768 this had definitely helped, thank you! however I was more referring to why in the differential form there has a changing pressure term although we have stated that pressure doesn't change for enthalpy. Is this because we are referring to the small fluctuations between states of the same ending pressure? In addition it doesn't seem obvious where this differential form would be applied, as normally for 2 states where entropy has changed we define the Delta change in enthalpy.
Absolutely incredible!!! I study physics in Romania and the system here is based on mechanical learning, no logic thinking, just learn like a computer. You just saved me man!!!
you literally saved my 1st semester. thank you
saved my p chem grade!! this man deserves many thousands of subs!! Excellent!!!
You desirve so much more recognition :) great job!
Your handwriting is superior, so nice to look at.
Thanks!
wow in second year of physics at QMUL and my teacher is so boring but you have just saved me
Haha thankyou! Glad I could help!
Thank you.
excellent explanation.
Love this playlist, U are single handedly saving my grade
Great to follow. remark: Going from R to kB implies that you go from an ensemble of particles to an average particle.
Essential is that the properties G, S, H, P, T are average values that do not change in time at equilibrium.
He fib.
Aje ,you made this course interesting for me
very clear explanation, thank you
Great video
Great explanation, thanks 💟
You’re welcome 😊
perfect!!!! congretulation
Thankyou!
Talk about other conjugated forces with a generalized potential, like suceptibility
Hi you said enthalpy is with constant pressure then how in the equation of enthalpy we are getting dp which is change of pressure so shouldn't that dp be zero??
amazing
Great explanation! Was wondering however the physical significance of our exact differential equations. For example dH= TdS +VdP, but we said that change in P for enthalpy is 0, so what's going on here?
So the purpose of defining enthalpy is so that we can have a change in an exact quantity that is good for circumstances in which pressure is constant. In the case of internal energy, dU = TdS + pdV the variables S and V directly correspond to a change in U, hence measuring the internal energy U is great for processes with constant volume and entropy, but less good for processes with constant pressure.
Defining enthalpy H = U + PV eliminates this, and we find that change in pressure dP corresponds directly to a change in enthalpy dH. Combining this with the first law of thermodynamics we can actually equate the change in heat energy, dQ (which is not an exact differential), to a change in enthalpy dH (which is an exact differential), provided that the pressure is constant (dp = 0). Hope that helps! :)
@@pazzy768 this had definitely helped, thank you! however I was more referring to why in the differential form there has a changing pressure term although we have stated that pressure doesn't change for enthalpy. Is this because we are referring to the small fluctuations between states of the same ending pressure? In addition it doesn't seem obvious where this differential form would be applied, as normally for 2 states where entropy has changed we define the Delta change in enthalpy.
Thank you 😀
This video is good in only the clearing of mathematical expressions but no one gives examples in Physical meaning
Pardon the question, but what program are you using to make this virtual chalkboard?
João Victor Notability for iPad !
Pazzy Boardman Thank you!
how do you get the equation in 15:08?
You mean c = n/V? That’s just the definition of molar concentration- the number of miles per unit volume!
No, i mean
μ1 - μ2 = RTln(C1/C2)