Notational question, d vs. delta when denoting an infintesimal change

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The discussion clarifies the distinction between the symbols "d" and "δ" in thermodynamics, specifically in the context of differentials. The symbol "d" represents exact differentials, applicable to defined properties or states such as internal energy (U) or entropy (S), while "δ" denotes inexact differentials for quantities like heat (Q) and work (W), which depend on the process rather than the state change. The equation dU = δQ + δW illustrates this relationship, emphasizing that inexact differentials cannot be determined solely by state changes. Understanding this distinction is crucial for accurate thermodynamic analysis.

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saminator910
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I have seen several thermodynamic equations represented with the lowercase delta, \delta, and the standard d to represent an infinitesimal change. For example, the change in internal energy is denoted in Wikipedia as:

dU = \delta Q + \delta W

Them the equation for \delta Q :

\delta Q = TdS

I just don't get when I should be inputting the \delta, and when to put in the d.
 
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saminator910 said:
I have seen several thermodynamic equations represented with the lowercase delta, \delta, and the standard d to represent an infinitesimal change. For example, the change in internal energy is denoted in Wikipedia as:

dU = \delta Q + \delta W

Them the equation for \delta Q :

\delta Q = TdS

I just don't get when I should be inputting the \delta, and when to put in the d.
There are a variety of ways to explain this.

One uses an exact differential when a defined property or state, such as U or S, changes. Q and W are quantities that depend on the process involved in the change in state of a system or surroundings. They do not relate to a change in property or state of a system or surroundings. Since these quantities cannot be determined from the change in state or property of the system or surroundings (eg. dU or dS) we use a different symbol (δQ and δW) which are referred to as inexact differentials.

It is not that the quantities represented by δQ and δW are really inexact for a given process. Rather the inexact differential just indicates that they cannot be determined by knowing the change in state.

AM
 
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Alright, thanks. I read up a little more about those and that makes sense, but I want to make sure I have this straight. So where df is the exact differential, it is though of as "net distance", displacement. On the other hand δf would be inexact, and thought of as the total distance. I have one more question, can I use standard integration on an inexact differential?
 
saminator910 said:
Alright, thanks. I read up a little more about those and that makes sense, but I want to make sure I have this straight. So where df is the exact differential, it is though of as "net distance", displacement. On the other hand δf would be inexact, and thought of as the total distance.
You could represent a change in displacement from an origin in moving from a particular point as an exact differential and the total path distance as an inexact differential.

I have one more question, can I use standard integration on an inexact differential?
If you know the path, you can use integration.

AM
 

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