I am currently taking applied thermodynamics at my university, and for the definition of entropy this is the formula used in the book (Thermodynamic for Engineers by Moran, Shapiro, Boettner, Bailey): $\text dS=\delta Q/T$. Here, the differential symbol $\text d$ is not used for the differential of $Q$. Can we define $\text dQ$ or similar expressions regarding energy, work, like $\text dW$, or $\text dE$?
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Related: https://physics.stackexchange.com/q/153791/2451 , https://physics.stackexchange.com/q/36150/2451 , https://physics.stackexchange.com/q/506194/2451 and links therein. – Qmechanic Apr 26 '22 at 10:18
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Have you covered work in mechanics yet? – BioPhysicist Apr 26 '22 at 10:23
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That is not the calculation of entropy change that Moran et al indicate. The integral of that quantity for an internally reversible process between two thermodynamic equilibrium states of a closed system is what they indicate as the change in entropy. And, they use the quantity $\delta Q$ to indicate that the differential amount of heat added to the system is a path-dependent quantity. So, in this context, what exactly is your question? – Chet Miller Apr 26 '22 at 11:24
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Does this answer your question? Why do we use different differential notation for heat and work? – Roger V. Apr 26 '22 at 11:34