Will E.

asked • 07/20/22

Approximation of a partial derivative

I am looking for a useful approximation for a partial derivative of the form

partial derivative of lnP with respect to lnA at constant S.

Suppose that P=1000 and A=200.

Suppose that I choose deltaP = 5 and deltaA = 0.5 and solve for P=1005 and A=200.5 at constant S.

Would the following then be a good approximation:

ln(P/(P+deltaP)) / ln(A/(A+deltaA)) and in which, in this example, would be

ln(1000/1005) / ln(200/200.5)

?

Roger R.

tutor
P is a function of A, and you can't choose P and A "independently." If you choose ΔA = +0.5, ΔP = P(200.5) -P(200).
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07/20/22

1 Expert Answer

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Ryan C. answered • 07/20/22

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Will E.

Wow! Thanks for that! I hope the following helps. I just used P and A to sort of clarify the partial. In fact, it is the partial derivative of LnP with respect to lnrho. I felt that lower case rho would look too much like a p so I used "A" instead. The LnP is actually Ln(Pressure), the Lnrho is actually the Ln(density) of a gas micture at specified pressure, temperature and entropy, and S is entropy. This is all about adiabtaic, isentropic expansion of gasses in a shifting equilibrium. What the partial actually is, is "y" (gamma; ratio of specific heats) but Not in the typically seen form of Cp/Cv (ratio of specific heats at constant pressure and constant volume) that is used in the so-called "frozen" equilibrium expansion of gasses (see Zucrow and Hoffman's "Gas Dynamics" Volume I, for example). The NASA CEA docs state that in a *shifting* equilibrium expansion, the Cp/Cv gamma must Not be used and instead gamma-sub-S where the partial's S denotes isentropic expansion (constant S). So, the P is just pressure, not a function, and rho (density) is a rather simple function of mass per unit volume at a given temperature and pressure. Does your approximation still work considering this? I can calculate the combustion products in equilibrium at an assigned pressure and a computed temperature (based on matching the reactants' and products' total enthalpy) and from this then determine its entropy. I can then slightly adjust the pressure and re-compute an equilibrium composition, but instead, at whatever slight change in temperature is required such that the entropy remains constant between the two cases. I suppose my poorly worded initial question should have included these details, that I just wish to be able to determine gamma-sub-S from these two closely-spaced pressures (P), two temperatures, two sets of product compositions, both at identical entropy, and two calculated densities (rho) from the preceding. On a side note, I have been trying to find ANYTHING ANYWHERE that will tell me why gamma-sub-S must be used instead of the "ordinary" gamma and have had zero luck. I need to dig further into the origins of the NASA CEA code that Gordon Sanford developed in the early 1960's. Always another nut to crack, isn't there? :)
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07/21/22

Ryan C.

Very cool stuff! Reminds me a lot of my grad school days in meteorology. :) I'm not certain that what I have to say will help you, but I'll throw in my two cents. In deriving the equation of state for adiabatic (or, equivalently, isentropic) processes in equilibrium, you assume that dq = 0 (i.e., that there is not exchange of heat between a parcel of gas and its surroundings) and that the process is quasi-static (or as you say "frozen"), meaning dw = pdV (i.e., the work performed by a parcel of gas on its surroundings) . When not in equilibrium, either dq =/= 0 or dw =/= pdV. If we stick still with adiabatic processes, then the only non-equilibrium process would be if dw =/= pdV, but then the work done by our parcel is no longer written in terms of state variables, making it process dependent. Perhaps this is why gamma must be modified appropriately depending on the nonequilibrium process at play.
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07/27/22

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