The discussion centers on the relationship between heat transfer (dQ), energy change (dE), and work done (dW) in quasi-static processes. It is established that for quasi-static processes, dW equals -dE, leading to the conclusion that dQ can equal zero under specific conditions. However, this does not apply to isothermal quasi-static processes, where dQ is not zero. The reference to Reif's "Fundamentals of Statistical and Thermal Physics" clarifies that the work done by the system is defined as dWr = -dEr, emphasizing that this relationship holds true primarily for adiabatic changes.
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Who says that this is the case for a quasi-static process? What about an isothermal quasi-static process, where dQ is not equal to zero?manhattan_project said:We know that dQ = dE + dW for any system.
However, in quasi-static processes, dW = -dE.
I don’t have a copy of that book. But, it dorsn’t sound correct to say that a system remains in a particular thermodynamic state if its internal energy changes. The equation you have written is correct only for an adiabatic change.manhattan_project said:I guess I am confused when dQ = 0.
In Reif's Fundamentals of Statistical and Thermal Physics, in Section 2.9 on quasi-static processes, it states that the work dW done by the system when it remains in a particular state r is defined as dWr = -dEr. I understood this as saying that dW = -dE for quasi-static processes